Chemistry 467 – Flashcards

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question
What kind of interactions occur when the Henry's law constant is greater than the pure vapor pressure?
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Unfavorable (repulsive) interactions
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The Raoult's law standard state is a physically realizable state
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True
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The Henry's law standard state is a physically realizable state
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False
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Fugacity is to pressure as activity is to (blank).
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Concentration
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What do we call the system when a reacting system has fully equilibrated?
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Equilibrium
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What is the heat of mixing for an ideal mixture?
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Zero
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If DeltaVmix is negative, what does that tell you about the interactions between the components of the mixture?
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They are generally favorable (attractive)
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Write the mathematical expression for chemical potential for a component in an ideal mixture
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mu=mu* + RT ln(x)
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If a mixture follows Raoult's Law, describe the interactions between the different molecules
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They are the same as between themselves (behaving as though pure)
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What happens to the boiling point of a mixture compared to the pure solvent (nonvolatile solute)?
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Rises
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Write the definition of chemical potential
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mu=(dG/dn)T,p,n
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At a given temperature and pressure, which phase is thermodynamically preferred?
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The one with the lowest chemical potential
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Write the fundamental equation of chemical thermodynamics
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dG=-SdT+VdP+sum(mudni)
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As pressure is increased, what happens to the boiling point of a liquid?
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It increases
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What property drives mixing for an ideal mixture?
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Entropy
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Does the Gibbs energy increase or decrease with an increase in pressure?
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Increases, because (dG/dP)T=V and V is positive
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If a reaction is exothermic, what happens to DeltarG if the temperature increases? Think Le Chatelier
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DeltarG will increase
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Why do we need fugacity
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To account for the behavior of real gases (attractions, repulsions)
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Under what conditions are two phases in equilibrium?
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When they have the same chemical potential (or molar Gibbs energy)
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What is the maximum number of phases that can coexist at a particular temperature and pressure?
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3
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Write the fundamental equation of thermodynamics
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dU=TdS-pdV
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Write the Gibbs equation (derived from the fundamental equation) for the Gibbs energy
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dG=-SdT+VdP
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What are the natural variables of the Gibbs energy?
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temperature and pressure
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Why is the Gibbs energy a useful quantity?
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It tells us the maximum non-expansion work a process can produce; how much of the energy is 'useful'
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Does the Gibbs energy increase or decreases as the temperature increases?
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Decreases, because dG/dT,p=-S
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How o you maximize the efficiency of a Carnot engine?
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Create the largest temperature difference between the hot and cold parts of the engine
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What is DeltaSuniverse fora phase transition at its normal transition temperature?
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0
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Briefly explain why all processes are treated as reversible for the surroundings
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Because the surroundings are infinitely massive compared to the system.
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Is DeltaSuniverse for a spontaneous, irreversible adiabatic expansion positive, negative, or zero?
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positive, the process is spontaneous
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Write the definition of Gibbs energy
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G=H-TS
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What is the sign of DeltavapH for any material?
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Positive, it takes an input of energy to vaporize something
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Write the thermodynamic definition of entropy
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dS=dqrev/T
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What makes a process spontaneous?
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DeltaSuniverse increases
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True or False: the entropy of the system can spontaneously decrease
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True
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True or False: the entropy of all substances is zero at zero Kelvin
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False
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What is DeltaU for any isothermal process involving ideal gas?
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Zero
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What is DeltaU for any cyclic process?
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Zero
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What do we mean when we say an expansion process is reversible?
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p=p,ex throughout the process, no net work for the process and its opposite
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Which process produces more work? reversible isothermal expansion of ideal gas or reversible adiabatic expansion of ideal gas?
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Reversible isothermal expansion of ideal gas produces more work
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When two objects are at different temperatures and then placed in thermal contact, in which direction does heat flow?
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from the hot to the cold
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On what variables does the internal energy of an ideal gas depend?
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Only on Temperature
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Write the total differential of internal energy as a function of temperature and volume, U(T,V)
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dU=(dU/dV),T*dV+(dU/dT),V*dT
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Write the definition of the constant volume heat capacity
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C,v=(dU/dT)v
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Write the definition of enthalpy
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H=U+pV
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What is meant by an adiabatic process?
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One in which no heat flows between system and surroundings.
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What cna a closed system exchange with the surroundings?
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Energy but not matter
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The Zeroth Law of Thermodynamics helps us to define what kind of Equilibrium?
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Thermal Equilibrium
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Generally speaking, what physical quantity is the First Law of Thermodynamics Concerned with?
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Energy, or internal energy
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Provide a brief explanation of the difference between heat and work at the molecular level?
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Work involves organized motion of the molecules; heat involved random motion
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Write the mathematical definition of expansion work
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dwexp=-pexdV
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Write the general expression for the chemical potential as a function of conditions.
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mu=mu^not+RTln(a)
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Write the general form of the reaction quotient, Q
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Q=product(a^nu)
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Write the relation between the equilibrium constant and the standard reaction Gibbs energy, DeltaGreaction
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DeltaGreaction^not=-RTln(K)
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What is the value of the reaction Gibbs energy when the reacting system is at equilibrium?
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DeltaGreaction=0
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If a reaction is exothermic, in what direction will it shift with an increase in temperature?
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Toward the reactants.
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True or False: The equilibrium composition of a gas phase reaction can change when the vessel is compressed at constant temperature.
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True
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True or False: The equilibrium constant of a gas phase reaction can change when the vessel is compressed at constant temperature.
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False
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True or False: The equilibrium constant of a reaction generally changes with temperature.
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True
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Write the general expression for the reaction Gibbs energy as a function of conditions
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DeltaGrxn=DeltaGrxn.not+RTln(Q)
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What is the key difference between standard conditions and standard biological conditions?
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Standard biological conditions are at pH 7, [H+]=1*10^-7 molar, 1 molar
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True or False: A transition state is a stable molecular configuration that can be isolated and studied
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False
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Is the mathematical shape of the transition state a maximum, minimum, or saddle point on the potential energy surface?
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Saddle Point
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To spectroscopically probe a transition state, what time scale of pulses do we need?
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Femtosecond
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What is the sign of DeltaS(doubledagger)?
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Negative
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What is the sign of DeltaG(doubledagger)?
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Positive
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List three state variables that we use to describe the physical properties of a gas?
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T,p,V and n
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The Zeroth Law of Thermodynamics defines what type of equilibrium?
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Thermal Equilibrium
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Name one of the scientists whose work led to the development of the ideal gas law?
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Boyle, Charles, Gay-Lussac, Avogadro
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Under what conditions of temperature and pressure do the ideal gas law hold true?
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Low pressure and high temperature
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Upon what was the development of the Ideal Gas Law based?
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Experimental observation and proposed principles
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What happens to the width of a probability distribution as the number of trials increases?
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The width narrows
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How do we calculate the average of a property described by a continuous probability density function?
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h_bar=integral(h*f(h)dh)=
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Define what is meant by an ensemble?
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A collection of individual items such as molecules
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Consider placing balls in boxes. We put 2 balls in the first box, 1 in the second, and 1 in the third. Assuming all the balls are identical, and the order doesn't matter, what is the statistical weight of this arrangement?
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W=4!/(2!1!1!)=12
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What is the statistical weight if all four balls are in the first box (of three)?
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W=4!/(4!0!0!)=1
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According to the principle of equal a priori probabilities, which of these two arrangements (all balls in one box or some in all three) is preferred?
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Neither is preferred
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State one of the constraints of the Boltzmann distribution
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Fixed number of molecules in the system; fixed total energy in the system
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State the two constraints that lead to the Boltzmann distribution
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Fixed number of molecules; fixed total energy in the system
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Write the mathematical expression of the partition function
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q=sum(e^-E_i/kT)
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Write the Boltzmann expression for entropy in terms of statistical weight
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S=kln(W)
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What does it mean when two states are said to be 'degenerate'?
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They have the same energy
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Consider a container of Ar gas. What happens to the average speed of the Ar atoms as the temperature increaseS?
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The average speed increases.
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At a molecular level, what is the source of the pressure of a gas?
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Collisions between the gas molecules and the walls of the container
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Consider two samples of gas, He and Ar, at the same temperature. In which sample are the atoms, on average, moving faster?
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He, the average speed increases as the mass decreases.
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State one of the assumptions in the kinetic molecular theory of gases, as we treated it.
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Molecules are in ceaseless, random motion; gas molecules have no size; all collisions are elastic.
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Describe what is meant by the term "mean free path"
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The average distance a molecule travels before experiencing a collision.
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What term do we use to describe the transfer of matter through another medium (such as a gas)?
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Diffusion
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If the pressure decreases, but the temperature stays the same, what happens to the collision density?
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The collision density decreases; there are fewer collisions.
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If there is a sharp change of concentration with distance, in what direction will diffusion occur?
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In the direction of the region with lower concentration.
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Name one other property besides diffusion that is correctly predicted by the kinetic molecular theory of gases:
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Viscosity, thermal conductivity
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What must phsyically happen between two molecules in order for a reaction to take place?
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Collision
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A reaction is found to have the rate law v=k[A]^2. What is the order of the reaction?
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Second order
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True or False: The rate of a reaction can be either positive or negative.
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False, reaction rates are always positive.
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At a molecular level, what does the activation energy represent?
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The minimum energy required for a collision to lead to reaction.
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True or False: If I know the overall reaction, I can write down the rate law?
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False, rate laws MUST be determined experimentally.
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What is meant by the term "half life"?
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The time it takes for the concentration of a reactant to drop by half the initial value.
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IF a reaction follows first order kinetic, how should I plot the data to determine the rate constant?
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As ln[A] vs. t
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If a reaction takes place through a bi-molecular mechanism, what order will the rate law be?
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Second order, of the form v=k[A][B]
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If we have a branching reaction that is under kinetic control, which product is more likely to be formed?
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The one with the larger rate constant.
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If we have a branching reaction that is under thermodynamic control, which product is more likely to be formed?
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The one with the larger equilibrium constant.
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In the steady state approximation, what do we assume about the concentration of an intermediate?
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The concentration does not change with time: d[I]/dt=0
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Briefly describe how a catalyst speeds up a reaction
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By lowering the activation energy, or providing an environment that allows the reactants to interact in a way that favors production of product.
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What step(s) generally determine the rate of reaction, fast or slow?
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Slow
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What kind of chemical species is commonly involved in chain reaction mechanisms?
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Free radicals
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In the Langmuir model, how deep can a surface be covered?
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One monolayer
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What is one of the two types of energy we have from Newtonian mechanics?
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Kinetic, potential
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Name one type of molecular motion that contributes to the heat capacity.
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Translational, vibrational, rotational.
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How much does each rotational degree of freedom contributes to the heat capacity?
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1/2R
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How many degrees of freedom does NH3 have?
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3N=12
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How many vibrational degrees of freedom does NH3 have?
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3N-6=6
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What quantity do we use as our 'energy ruler' in determining whether an energy state is high or low
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The quantity k.bT (or RT in molar units)
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Name or describe one phenomenon that led to the development of quantum mechanics?
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Blackbody radiation, heat capacity of solids, photoelectric effect, electron diffraction
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What did Einstein's explanation of the photoelectric effect tell us about light?
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Light can act like a particle, or the energy is quantized.
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What was de Broglie's hypothesis about the behavior of particles?
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Particles should behave like waves to some degree
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Name an experiment that proved de Broglie correct?
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Electron diffraction, two-slit experiment
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How do we mathematically describe the behavior of a particle in quantum mechanics?
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With a wavefunction
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What does the Hamiltonian operator account for?
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Total energy, kinetic plus potential
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What does the quantity psi*psi tell us about?
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The probability of finding the particle between x and x+dx
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State one of the requirement of a wavefunction?
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Continuous, continuous first derivative, square integrable, single valued, finite
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If we have a free particle (no forces acting on it) that is described by a single value of momentum, where is the particle located?
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It has no location, it is delocalized over all space
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In the formalism of quantum mechanics, how do we represent a physically measurable quantity?
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With the corresponding quantum mechanical operator.
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How do we determine the expectation value of a physically observable quantity?
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Evaluate =integral(psi*j_hat*psi d(tao)
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If a wavefunction is not an eigenfunction of a given operator, how should I write it?
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As a linear combination of eigenfunctions of that operator.
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If a wavefunction is a linear combination of two eigenfunctions of the Hamiltonian, what values of energy can we measure?
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We can only measure one of the two eigenvalues.
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True or False: Before an individual measurement on the wavefunction (in this case, a linear combination of two eigenfunctions of the Hamiltonian), I can predict the energy I will measure.
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False: I can predict the probability of each measurement, but not individual measurements.
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After measuring the energy of the wavefunction in question 2, what happens to the wavefunction?
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The wavefunction 'collapses' to the eigenfunction corresponding to the measured energy.
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What does it mean to say that two operators do not commute?
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The result of the measurements will be different depending on the order in which the measurements are performed.
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What is a postulate?
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Something we assume to be true and use for further reasoning.
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For the particle in a box, what happens to the energy as the size of the box decreases?
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Energy increases.
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For the n=1 state of the particle in a box, what is probability of finding the right particle right next to the wall of the box?
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Zero
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True or False: A particle confined to a box can have zero energy
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False; if the energy is zero, there is no particle in the box.
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If I want to cause a transition between two energy states, what must the frequency of the incident light be?
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v=DeltaE/h; the incident light has to match the difference in energy of the two states.
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What are the two conditions that must be met for a spectroscopic transition to occur?
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The energy of the photon must match the energy difference between the states. The transition dipole moment must be non-zero; the transition must be allowed.
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In the classical limit, what does the probability density function look like for the particle in a box?
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Uniform probability of finding the particle anywhere in the box.
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Why don't we worry about quantum effects when talking about an ideal gas?
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The size of the container is so large that the energy levels can be treated as a continuum; or the molecules are so far apart that they don't have any quantum interactions.
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State one practical application of tunneling
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Schottky or tunneling diode; proton transfer; nuclear fusion; electron microscopy
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Which are more likely to tunnel through a barrier, electrons or protons?
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Electrons, because of their smaller mass.
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True or false: After tunneling through a barrier, a particle has less kinetic energy
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False; the energy is unchanged. The amplitude of the wavefunction, or the probability of being on the other side of the barrier, is reduced.
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If we isotopically substitute deuterium for hydrogen, and the rate of reaction decreases, what does that tell us about the rate limiting step?
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It likely involves proton transfer, or proton tunneling.
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In a 3-D situation, what aspect of the system leads to degenerate states?
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Symmetry
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In addition to energy, the rigid rotor illustrates that what physical quantity is also quantized?
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Angular momentum
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In what region of the electromagnetic spectrum do rotational transitions take place?
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The microwave region
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How can we break the degeneracy of rotational states?
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With an external field, magnetic or electric.
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TRue or False: Compared to k.bT, rotational levels are close together?
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True
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Name one type of spectroscopy that allows us to measure vibrational transitions.
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IR or Raman spectroscopy
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How many vibrational normal modes does H2O have?
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3n-6=3
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True or False: a molecule can have no vibrational energy?
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False, there is always zero point energy of 1/2 h*nu
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In what region of the electromagnetic spectrum do vibrational transitions take place?
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Infrared
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True or False: Compared to k.bT, vibrational levels are very close together?
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False
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True or False: Electrons circle the nucleus just like planets orbit the sun.
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False
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Name one atom for which we have solve the Schrodinger equation exactly.
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Hydrogen (it's the only one)
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What do we call solutions to the Schrodinger equation for the hydrogen atom?
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Atomic orbitals
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In what range of the electromagnetic spectrum do we observe transitions between the electronic states of an atom?
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Visible to UV
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What do we take as our zero of potential energy for a hydrogen atom?
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Infinite separation of the proton and electron
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When constructing molecular orbitals from atomic orbitals, h ow many molecular orbitals will we have?
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The same as the number of atomic orbitals.
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We generally talk about two types of molecular orbitals. Name one.
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sigma and pi
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Why doesn't He form a diatomic molecule?
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The energy would have higher than for two unbonded atoms.
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True or False: All molecular orbitals are localized along particular bonds
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False: Most molecular orbitals are delocalized over the whole molecule.
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How does the Born-Oppenheimer approximation treat motion of the nuclei?
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Nuclei move much more slowly than the electrons.
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True or False: If a molecule has a bound ground electronic state, all excited states are also bound.
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False: Excited states can be unbound. The molecule will dissociate if it is excited to such a state.
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Name one process by which an electronically excited molecule relaxes and emits a photon.
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Fluorescence, phosphorescence, chemiluminescence.
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What has a longer lifetime, fluorescence or phosphorescence?
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Phosphorescence
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Why are the lifetimes different for fluorescence and phosphorescence?
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Because phosphorescence involves a forbidden transition.
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What term do we use to describe breaking chemical bonds with light?
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Photolysis or photodissociation
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Will fluorescence occur at longer or shorter wavelengths than the excitation?
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Longer wavelengths, or lower energy
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What quantum mechanical model do we use for translations of molecules when building the partition function?
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Particle in a box
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identify one of the key components of a laser:
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Gain medium, pump source, resonator cavity
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True or False: at room temperature, we can reasonable assume that rotational levels are close together
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True: the rotational temperature is many times less than T
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At the molecular level, what conditions are required for ideal behavior?
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No interactions (except for collisions)
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What do we call a collection of individual microsystems?
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An ensemble
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Given our collection of microsystems, how do we determine bulk properties?
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By taking the ensemble average of that property: M_bar=sum(M_j*P_J)=(sum(M_j*e^(-E_j/kT)))/Q
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What thermodynamic properties do we keep constant in the canonical ensemble?
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N,V, and T
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What is the interaction potential for an ideal gas?
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E_p=0 (or V=o)
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What do we call the temperature below which a gas can condense?
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The critical temperature
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Write the definition of the reduced temperature.
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T_r=T/T_c
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Name one equation of state for real gases
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van der Waals, virial (Berthelot, Dieterici, Redlich-Kwong)
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What happens when a real gas is compressed at a temperature below the critical temperature?
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It condenses
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What do the two parameters in the van der Waals equation account for?
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Finite volume of the gas molecules and attractive interactions
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For a particular gas at ambient in the van der Waals equation account for?
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Attractive interactions
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According to the principle of corresponding states, how do we best compare the behavior of different gases?
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By comparing the reduced variables
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In terms of molecular order, what characterizes the structure of a liquid at short and long distances?
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Short-range order, long range disorder
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What can a closed system exchange with its surroundings?
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Energy, but not matter
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The zeroth law of thermodynamics helps us to define what kind of equilibrium?
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Thermal
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Generally speaking, what physical quantity is the First Law of Thermodyamics concerned with?
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Energy, or internal energy
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Provide a brief explanation of the difference between heat and work at the molecular level?
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Work involves organized motion of the molecules, heat involves unorganized motion.
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Give the mathematical definition of expansion work?
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delW_exp=-p_ex*dV
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On what variables does the internal energy of an ideal gas depend?
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Only T
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Write the total differential of internal energy as a function of temperature and volume U(T,V)
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dU=(dU/dV)_T*dV+(dU/dT)_v*dT
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Write the definition of constant volume heat capacity
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C_v=(dU/dT)_v
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Write the definition of enthalpy
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H=U+pV
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What is meant by an adiabatic process
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One in which no heat flows between system and surroundings.
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