Chemistry Chapter 13 Conceptual Questions – Flashcards

Identify the methods used to monitor a reaction as it occurs in the reaction flask. A) polarimeter B) spectrometer C) pressure measurement D) none of the above E) all of the above

Give the characteristic of a first order reaction having only one reactant. A) The rate of the reaction is not proportional to the concentration of the reactant. B) The rate of the reaction is proportional to the square of the concentration of the reactant. C) The rate of the reaction is proportional to the square root of the concentration of the reactant. D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. E) The rate of the reaction is directly proportional to the concentration of the reactant.

Give the characteristic of a zero order reaction having only one reactant. A) The rate of the reaction is not proportional to the concentration of the reactant. B) The rate of the reaction is proportional to the square of the concentration of the reactant. C) The rate of the reaction is proportional to the square root of the concentration of the reactant. D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. E) The rate of the reaction is directly proportional to the concentration of the reactant

Give the characteristic of a second order reaction having only one reactant. A) The rate of the reaction is not proportional to the concentration of the reactant. B) The rate of the reaction is proportional to the square of the concentration of the reactant. C) The rate of the reaction is proportional to the square root of the concentration of the reactant. D) The rate of the reaction is proportional to the natural logarithm of the concentration of the reactant. E) The rate of the reaction is directly proportional to the concentration of the reactant.

What is the overall order of the following reaction, given the rate law? NO(g) + O3(g) → NO2(g) + O2(g) Rate = k[NO][O3]

What are the units of k in the following rate law? Rate = k[X][Y]2

What are the units of k in the following rate law? Rate = k[X]2[Y]2

What are the units of k in the following rate law? Rate = k[X][Y]

What are the units of k in the following rate law? Rate = k[X]0[Y]0

What are the units of k in the following rate law? Rate = k[X][Y]1/2

What are the units of k in the following rate law? Rate = k[X]2

Which of the following represents the integrated rate law for a first-order reaction? A) ln([A]t/[A]o) = - kt B) (1/[A]t) - (1/[A]o] = kt C) [A]t - [A]o = - kt D) k = Ae(-Ea/RT) E) ln(k2/k1) = Ea/R (1/T ) + lnA

Which of the following represents the integrated rate law for a second-order reaction? A) ln([A]t/[A]o) = - kt B) (1/[A]t) - (1/[A]o] = kt C) [A]t - [A]o = - kt D) k = Ae(-Ea/RT) E) ln(k2/k1) = Ea/R (1/T ) + lnA

Which of the following represents the integrated rate law for a zeroth-order reaction? A) ln([A]t/[A]o) = - kt B) (1/[A]t) - (1/[A]o] = kt C) [A]t - [A]o = - kt D) k = Ae(-Ea/RT) E) ln(k2/k1) = Ea/R (1/T ) + lnA

What data should be plotted to show that experimental concentration data fits a first-order reaction? A) 1/[reactant] vs. time B) [reactant] vs. time C) ln[reactant] vs. time D) ln(k) vs. 1/T E) ln(k) vs. Ea

What data should be plotted to show that experimental concentration data fits a second-order reaction? A) ln[reactant] vs. time B) [reactant] vs. time C) ln(k) vs. 1/T D) 1/[reactant] vs. time E) ln(k) vs. Ea

What data should be plotted to show that experimental concentration data fits a zeroth-order reaction? A) ln[reactant] vs. time B) 1/[reactant] vs. time C) ln(k) vs. 1/T D) ln(k) vs. Ea E) [reactant] vs. time

Which of the following statements is FALSE? A) The average rate of a reaction decreases during a reaction. B) It is not possible to determine the rate of a reaction from its balanced equation. C) The rate of zero order reactions are not dependent on concentration. D) The half life of a first order reaction is dependent on the initial concentration of reactant. E) None of the statements are FALSE.

Which of the following statements is FALSE? A) The half life of a zero order reaction is dependent on concentration. B) The half life of a second order reaction is not dependent on concentration. C) The rate of second order reactions is dependent on concentration. D) The rate of a first order reaction is dependent on concentraion. E) None of the statements are FALSE.

For a reaction, what generally happens if the temperature is increased? A) a decrease in k occurs, which results in a faster rate B) a decrease in k occurs, which results in a slower rate C) an increase in k occurs, which results in a faster rate D) an increase in k occurs, which results in a slower rate E) there is no change with k or the rate

Identify the rate-determining step. A) the slowest step B) the faster step C) the fast step D) always the last step E) always the second step

Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction) Mechanism: A2 ⇌ 2A fast A + B → AB slow

Which of the following statements is TRUE? A) The rate constant does not depend on the activation energy for a reaction where the products are lower in energy than the reactants. B) A catalyst raises the activation energy of a reaction. C) Rate constants are temperature dependent. D) The addition of a homogeneous catalyst does not change the activation energy of a given reaction. E) None of the above are true.

Identify an homogeneous catalyst. A) SO2 over vanadium (V) oxide B) Pd in H2 gas C) Pt with methane D) H2SO4 with concentrated HCl E) N2 and H2 catalyzed by Fe

Identify an heterogeneous catalyst. A) CFCs with ozone B) Pd in H2 gas C) KI dissolved in H2O2 D) H2SO4 with concentrated HCl E) H3PO4 with an alcohol

In the hydrogenation of double bonds, a catalyst is needed. In the first step, the reactants must come into contact with a metal surface. This step is known as ________. A) adsorption B) diffusion C) reaction D) desorption E) none of the above

In the hydrogenation of double bonds, a catalyst is needed. In the last step, the reactants must escape from the surface into the gas phase. This step is known as ________. A) adsorption B) diffusion C) reaction D) desorption E) none of the above

Biological catalysts that increase the rates of biochemical reactions are known as ________. A) substrates B) inhibitors C) enzymes D) binders E) trumanettes

What is the overall order of the following reaction, given the rate law? X + 2 Y → 4 Z Rate = k[X][Y]

What are the units of k in a zero order reaction?

What are the units of k in a first order reaction?

What are the units of k in a second order reaction?

What is the overall order of the following reaction, given the rate law? 2 X + 3 Y → 2 Z Rate = k[X]1[Y]2

What is the overall order of the following reaction, given the rate law? 2NO(g) + H2(g) → N2(g) + 2H2O(g) Rate = k[NO]2[H2]

Which of the following represents the equation for a first-order half-life?

Which of the following represents the equation for a second-order half-life?

Which of the following represents the equation for a zero-order half-life?

How many half-lives are required for the concentration of reactant to decrease to 25% of its original value? A) 1 B) 4 C) 1.5 D) 3.5 E) 2

How many half-lives are required for the concentration of reactant to decrease to 12.5% of its original value? A) 3 B) 2 C) 2.5 D) 2.75 E) 8

How many half-lives are required for the concentration of reactant to decrease to 1.56% of its original value? A) 6 B) 4 C) 24 D) 6.5 E) 7.5

If the concentration of a reactant is 6.25%, how many half-lives has it gone through? A) 7 B) 10 C) 3 D) 4 E) 5

Which of the following reactions would you predict to have the smallest orientation factor? A) X2 + Y2 → 2 XY B) NOCl2 + NO → 2 NOCl C) N2 + O2 → 2 NO D) N + O2 → NO2 E) All of these reactions should have nearly identical orientation factors.

Which of the following reactions would you predict to have the largest orientation factor? A) NOCl(g) + NOCl(g) → 2NO(g) + Cl2(g) B) Br2(g) + H2C=CH2(g) → H2BrC-CBrH2(g) C) NH3(g) + BCl3(g) → H3N-BCl3(g) D) H(g) + F(g) → HF(g) E) All of these reactions should have nearly identical orientation factors.

Which rate law is termolecular? A) rate = k[A][B]2 B) rate = k [A][B]3 C) rate = k [A]5 D) rate = k [A][B][C][D] E) rate = k [A]2

Which rate law is bimolecular? A) rate = k[A][B]3 B) rate = k [A][B] C) rate = k [A]3 D) rate = k [A][B][C][D] E) rate = k [A]2[B]2

Given the following proposed mechanism, predict the rate law for the overall reaction. 2NO2 + Cl2 → 2NO2Cl (overall reaction) Mechanism NO2 + Cl2 → NO2Cl + Cl slow NO2 + Cl → NO2Cl fast A) Rate = k[NO2][Cl2] B) Rate = k[NO2]2[Cl2]2 C) Rate = k[NO2][Cl] D) Rate = k[NO2Cl][Cl]2 E) Rate = k[NO2Cl]2