Chapter 4 , 5 , 6 Terms – Flashcards

A system that does no work but which transfers heat to the surroundings has A) q < 0, ∆E > 0 B) q < 0, ∆E < 0 C) q > 0, ∆E > 0 D) q > 0, ∆E < 0 E) q < 0, ∆E = 0

A system that does no work but which receives heat from the surroundings has A) q < 0, ∆E > 0 B) q > 0, ∆E < 0 C) q = ∆E D) q = -∆E E) w = ∆E

A system which undergoes an adiabatic change (i.e., q = 0) and does work on the surroundings has A) w < 0, ∆E = 0 B) w > 0, ∆E > 0 C) w > 0, ∆E < 0 D) w < 0, ∆E > 0 E) w < 0, ∆E < 0

A system which undergoes an adiabatic change (i.e., q = 0) and has work done on it by the surroundings has A) w = ∆E B) w = -∆E C) w > 0, ∆E < 0 D) w < 0, ∆E > 0 E) w > ∆E

A system receives 575 J of heat and delivers 425 J of work. Calculate the change in theinternal energy, E, of the system. A) -150 J B) 150 J C) -l000 J D) 1000 J E) 575 J

A system delivers 225 J of heat to the surroundings while delivering 645 J of work. Calculate the change in the internal energy, ∆E, of the system. A) -420 J B) 420 J C) -870 J D) 870 J E) -225 J

A system delivers 1275 J of heat while the surroundings perform 855 J of work on it. Calculate ∆E in J. A) -2130 J B) -420 J C) 420 J D) 2130 J E) -1275 J

A system absorbs 21.6 kJ of heat while performing 6.9 kJ of work on the surroundings. If the initial internal energy, E, is 61.2 kJ, what is the final value of E? A) 32.7 kJ B) 46.5 kJ C) 75.9 kJ D) 82.8 kJ E) 89.7 kJ

A system initially has an internal energy E of 501 J. It undergoes a process during which it releases 111 J of heat energy to the surroundings, and does work of 222 J. What is the final energy of the system, in J? A) 168 J B) 390 J C) 612 J D) 834 J E) It cannot be calculated without more information.

A system expands from a volume of 1.00 L to 2.00 L against a constant external pressure of 1.00 atm. The work (w) done by the system, in J, is A) 1.00 J B) 2.00 J C) 1.01 x 10²J D) 1.01 x 10⁵j E) None of these choices is correct.

A system contracts from an initial volume of 15.0 L to a final volume of 10.0 L under a constant external pressure of 0.800 atm. The value of w, in J, is A) -4.0 J B) 4.0 J C) -405 J D) 405 J E) 4.05 x 10³J

An ideal gas (the system) is contained in a flexible balloon at a pressure of 1 atm and is initially at a temperature of 20.°C. The surrounding air is at the same pressure, but its temperature is 25°C. When the system has equilibrated with its surroundings, both systems and surroundings are at 25°C and 1 atm. In changing from the initial to the final state, which one of the following relationships regarding the system A) ∆E < 0 B) ∆E = 0 C) ∆H = 0 D) w > 0 E) q > 0

Which one of the following relationships is always correct? A) potential energy + kinetic energy = constant B) E = q + w C) ∆E = ∆H - P∆V D) H = E + PV E) ∆H = qv

Cold packs, whose temperatures are lowered when ammonium nitrate dissolves in water, are carried by athletic trainers when transporting ice is not possible. Which of the following is true of this reaction? A) ∆H < 0, process is exothermic B) ∆H > 0, process is exothermic C) ∆H < 0, process is endothermic D) ∆H > 0, process is endothermic E) ∆H = 0, since cold packs are sealed

The dissolution of barium hydroxide in water is an exothermic process. Which of the following statements is correct? A) The enthalpy of solid barium hydroxide plus pure water is less than that of the solution, at the same temperature. B) The enthalpy of solid barium hydroxide plus pure water is greater than that of the solution, at the same temperature. C) The enthalpy of solid barium hydroxide plus pure water is the same as that of the solution, at the same temperature. D) The temperature of the solution is lower than of the barium hydroxide and water before mixing. E) When barium hydroxide dissolves in water, the system does work on the surroundings.

Two solutions (the system), each of 25.0 mL volume and at 25.0°C, are mixed in a beaker. A reaction occurs between them, and the temperature rises to 35.0°C. After the products have equilibrated with the surroundings, the temperature is again 25.0°C and the total volume is 50.0 mL. No gases are involved in the reaction. Which one of the following relationships concerning the change from initial to final states (both at 25.0°C) is correct? A) ∆E = 0 B) ∆H = 0 C) ∆E > 0 D) q = 0 E) w = 0

A Snickers® candy bar contains 280 Calories, of which the fat content accounts for 120 Calories. What is the energy of the fat content, in kJ? A) 5.0 x 10⁻¹ kJ B) 29 kJ C) 5.0 x 10² kJ D) 1.2 x 10³ kJ E) 5.0 x 10⁵ kJ

Your favorite candy bar, Gummy Beakers, contains 1.2 x 10⁶ J of energy while your favorite soft drink, Bolt, contains 6.7 x 10⁵ J. If you eat two packs of Gummy Beakers a day and drink 3 cans of Bolt, what percent of your 2000 Calorie daily food intake is left for broccoli, beans, beef, etc.? A) 53% B) 47% C) 27% D) 11% E) 0%

Natural gas, or methane, is an important fuel. Combustion of one mole of methane releases 802.3 kilojoules of energy. How much energy does that represent in kilocalories? A) 1.92 x 10⁻¹ kcal B) 1.92 x 10² kcal C) 3.36 x 10³ kcal D) 1.92 x 10⁵ kcal E) 3.36 x 10⁶ kcal

Which of the following is not a state function? A) internal energy B) volume C) work D) pressure E) enthalpy

Calculate q when 28.6 g of water is heated from 22.0°C to 78.3°C. A) 0.385 kJ B) 1.61 kJ C) 6.74 kJ D) 9.37 kJ E) 1.61 x 10³ kJ

If, as a pioneer, you wished to warm your room by taking an object heated on top of a pot-bellied stove to it, which of the following 15-pound objects, each heated to 100°C, would be the best choice? The specific heat capacity (in J/(g·K)) for each substance is given in parentheses. Iron (0.450), copper (0.387), granite (0.79), gold (0.129), water (4.18). A) iron B) copper C) granite D) gold E) water

Ethylene glycol, used as a coolant in automotive engines, has a specific heat capacity of 2.42 J/(g·K). Calculate q when 3.65 kg of ethylene glycol is cooled from 132°C to 85°C. A) -1900 kJ B) -420 kJ C) -99 kJ D) -0.42 kJ E) -4.2 x 10⁻⁶ kJ

A 275-g sample of nickel at l00.0°C is placed in 100.0 mL of water at 22.0°C. What is the final temperature of the water? Assume that no heat is lost to or gained from the surroundings. Specific heat capacity of nickel = 0.444 J/(g·K) A) 39.6°C B) 40.8°C C) 61.0°C D) 79.2°C E) 82.4°C

Benzene is a starting material in the synthesis of nylon fibers and polystyrene (styrofoam). Its specific heat capacity is 1.74 J/(g·K). If 16.7 kJ of energy is absorbed by a 225-g sample of benzene at 20.0°C, what is its final temperature? A) -22.7°C B) 36.7°C C) 42.7°C D) 62.7°C E) None of these choices is correct.

When Karl Kaveman adds chilled grog to his new granite mug, he removes 10.9 kJ of energy from the mug. If it has a mass of 625 g and was at 25°C, what is its new temperature? Specific heat capacity of granite = 0.79 J/(g·K) A) 3°C B) 14°C C) 22°C D) 47°C E) None of these choices is correct.

The Starship Enterprise is caught in a time warp and Spock is forced to use the primitive techniques of the 20th century to determine the specific heat capacity of an unknown mineral. The 307-g sample was heated to 98.7°C and placed into a calorimeter containing 72.4 g of water at 23.6°C. The heat capacity of the calorimeter was 15.7 J/K. The final temperature in the calorimeter was 32.4°C. What is the specific heat capacity of the mineral? A) 0.124 J/(g·K) B) 0.131 J/(g·K) C) 0.138 J/(g·K) D) 0.145 J/(g·K) E) None of these choices is correct.ⁿ

A piece of copper metal is initially at 100.0°C. It is dropped into a coffee cup calorimeter containing 50.0 g of water at a temperature of 20.0°C. After stirring, the final temperature of both copper and water is 25.0°C. Assuming no heat losses, and that the specific heat (capacity) of water is 4.18 J/(g·K), what is the heat capacity of the copper in J/K? A) 2.79 J/K B) 3.33 J/K C) 13.9 J/K D) 209 J/K E) None of these choices is correct.

A common laboratory reaction is the neutralization of an acid with a base. When 50.0 mL of 0.500 M HCl at 25.0°C is added to 50.0 mL of 0.500 M NaOH at 25.0°C in a coffee cup calorimeter, the temperature of the mixture rises to 28.2°C. What is the heat of reaction per mole of acid? Assume the mixture has a specific heat capacity of 4.18J/(g·K) and that the densities of the reactant solutions are both 1.00 g/mL. A) 670 J B) 1300 J C) 27 kJ D) 54 kJ E) > 100 kJ

Sand is converted to pure silicon in a three step process. The third step is SiCl₄(g) + 2Mg(s) → 2MgCl₂(s) + Si(s) ∆H = -625.6 kJ What is the enthalpy change when 25.0 mol of silicon tetrachloride is converted to elemental silicon? A) -25.0 kJ B) -7820 kJ C) -1.56 x 10⁴ kJ D) -3.13 x 10⁴ kJ E) None of these choices is correct.

Calcium hydroxide, which reacts with carbon dioxide to form calcium carbonate, was used by the ancient Romans as mortar in stone structures. The reaction for this process is Ca(OH)₂(s) + CO₂(g) → CaCO₃(s) + H₂O(g) ∆H = -69.1 kJ What is the enthalpy change if 3.8 mol of calcium carbonate is formed? A) -18 kJ B) -69 kJ C) -73 kJ D) -260 kJ E) None of these choices is correct.

32. Galena is the ore from which elemental lead is extracted. In the first step of the extraction process, galena is heated in air to form lead(II) oxide. 2PbS(s) + 3O₂(g) → 2PbO(s) + 2SO₂(g) ∆H = -827.4 kJ What mass of galena is converted to lead oxide if 975 kJ of heat are liberated? A) 203 g B) 282 g C) 406 g D) 478 g E) 564 g

The highly exothermic thermite reaction, in which aluminum reduces iron(III) oxide to elemental iron, has been used by railroad repair crews to weld rails together. 2Al(s) + Fe₂O₃(s) → 2Fe(s) + Al₂O₃(s) ∆H = -850 kJ What mass of iron is formed when 725 kJ of heat are released? A) 47 g B) 65 g C) 95 g D) 112 g E) 130 g

Use Hess's Law to calculate the enthalpy change for the reaction WO₃(s) + 3H₂(g) → W(s) + 3H₂O(g) from the following data: 2W(s) + 3O₂(g) → 2WO₃(s) ∆H = -1685.4 kJ 2H₂(g) + O₂(g) → 2H₂O(g) ∆H = -477.84 kJ A) 125.9 kJ B) 252.9 kJ C) 364.9 kJ D) 1207.6 kJ E) None of these choices is correct.

Calculate the enthalpy change for the reaction NO(g) + O(g) → NO₂(g) from the following data: NO(g) + O₃(g) → NO₂(g) + O₂(g) ∆H = -198.9 kJ O₃(g) → 1.5O₂(g) ∆H = -142.3 kJ O₂(g) → 2O(g) ∆H = 495.0 kJ A) -551.6 kJ B) -304.1 kJ C) 190.9 kJ D) 153.8 kJ E) 438.4 kJ

Use the following data to calculate the standard heat (enthalpy) of formation, ∆H°f , of manganese(IV) oxide, MnO2 (s). 2MnO₂(s) → 2MnO(s) + O₂(g) ∆H = 264 kJ MnO2(s) + Mn(s) → 2MnO(s) ∆H = -240 kJ A) -504 kJ B) -372 kJ C) -24 kJ D) 24 kJ E) 504 kJ

Which one of the following statements about standard states is incorrect? A) The standard state of a solid compound is the pure solid. B) The standard state of a liquid compound is the pure liquid. C) The standard state of a gaseous compound is the gas at a pressure of 1 atmosphere. D) The standard state of an aqueous solute is a saturated solution in water. E) The standard state of an element is the form in which it is stable at 1 atm and a specified temperature, usually 25°C.

Which one of the following equations represents the formation reaction of CH3OH(l)? A) C(g) + 2H₂(g) + 1/2O₂(g) → CH₃OH(l) B) C(g) + 4H(g) + O(g) → CH₃OH(l) C) C(graphite) + 4H(g) + O(g) → CH₃OH(l) D) C(diamond) + 4H(g) + O(g) → CH₃OH(l) E) C(graphite) + 2H₂(g) + O₂(g) → CH₃OH(l)

Which one of the following is not a correct formation reaction? (products are correct) A) H₂(g) + O(g) → H₂O(l) B) 1/2H₂(g) + 1/2Cl₂(g) → HCl(g) C) 6C(graphite) + 3H₂(g) → C₆H₆(l) D) C(graphite) → C(diamond) E) 6C(graphite) + 6H₂(g) + 3O₂(g) → C₆H₁₂O₆(s)

Which one of the following is a correct formation reaction? A) C(diamond) → C(graphite) B) H₂(g) + O(g) → H₂O(l) C) C(graphite) + 4H(g) → CH₄(g) D) 6C(graphite) + 6H₂O(s) → C₆H₁₂O₆(s) E) 2C(graphite) + 3H₂(g) + O₂(g) → C₂H₅OH(l)

Calculate the ∆H°rxn for the decomposition of calcium carbonate to calcium oxide and carbon dioxide. ∆H°f [CaCO₃(s)] = -1206.9 kJ/mol; ∆H°f [CaO(s)] = -635.1 kJ/mol; ∆H°f [CO₂(g)] = -393.5 kJ/mol CaCO₃(s) → CaO(s) + CO₂(g) A) -2235.5 kJ B) -1448.5 kJ C) -178.3 kJ D) 178.3 kJ E) 2235.5 kJ

Nitric acid, which is among the top 15 chemicals produced in the United States, was first prepared over 1200 years ago by heating naturally occurring sodium nitrate (called saltpeter) with sulfuric acid and collecting the vapors produced. Calculate ∆H°rxn for this reaction. ∆H°f [NaNO₃(s)] = -467.8 kJ/mol; ∆H°f [NaHSO₄(s)] = -1125.5 kJ/mol; ∆H°f[H₂SO₄(l) = -814.0 kJ/mol; ∆H°f [HNO₃(g)] = -135.1 kJ/mol NaNO₃(s) + H2SO₄(l) → NaHSO₄(s) + HNO₃(g) A) -644.2 kJ B) -291.4 kJ C) -21.2 kJ D) 21.2 kJ E) 644.2 kJ

An important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide. ∆H°f [NH₃(g)] = -45.9 kJ/mol; ∆H°f [NO(g)] = 90.3 kJ/mol; ∆H°f [H₂O(g)] = -241.8 kJ/mol 4NH₃(g) + 5O₂(g) 4NO(g) + 6H₂O(g) Calculate ∆H°rxn for this reaction. A) -906.0 kJ B) -197.4 kJ C) -105.6 kJ D) 197.4 kJ E) 906.0 kJ

Calculate the ∆H°rxn for the following reaction. ∆H°f [SiO2(s)] = -910.9 kJ/mol; ∆H°f [SiCl₄(g)] = -657.0 kJ/mol; ∆H°f [HCl(g)] = -92.3 kJ/mol; ∆H°f [H₂O (g)] = -241.8 kJ/mol SiO₂(s) + 4HCl(g) SiCl₄(g) + 2H₂O(g) A) -139.5 kJ B) -137.4 kJ C) -104.4 kJ D) 104.4 kJ E) 139.5 kJ

Calculate the ∆H°rxn for the following reaction. ∆H°f [AsH3(g)] = 66.4 kJ/mol; ∆H°f [H3AsO4(aq)] = -904.6 kJ/mol; ∆H°f [H2O(l)] = -285.8 kJ/mol H3AsO₄(aq) + 4H₂(g) → AsH₃(g) + 4H₂O(l) A) -1981.4 kJ B) -685.2 kJ C) -172.2 kJ D) 172.2 kJ E) 685.2 kJ

Ethanol, C₂H₅OH, is being promoted as a clean fuel and is used as an additive in many gasoline mixtures. Calculate the ∆H°rxn for the combustion of ethanol. ∆H°f [C₂H₅OH(l)] = -277.7 kJ/mol; ∆H°f [CO₂(g)] = -393.5 kJ/mol; ∆H°f [H₂O(g)] = -241.8 kJ/mol A) -1234.7 kJ B) -751.1 kJ C) -357.6 kJ D) 357.6 kJ E) 1234.7 kJ

(T/F) The only way in which a system can do work on the surroundings is by expansion against the external pressure.

(T/F) Different chemical bonds have different potential energies.

(T/F) For a reaction in a sealed, rigid container, ∆H is always greater than ∆E.

(T/F) ∆H does not depend on the path of a reaction, but ∆E does.

(T/F) The enthalpy (H) of liquid water is greater than that of the same quantity of ice at the same temperature.

(T/F) In an endothermic reaction, in going from the reactants to the products at the same temperature, the value of q is negative.

(T/F) ∆E values obtained by bomb calorimetry can be converted to give accurate ∆H values.

(T/F) The standard state of a substance in aqueous solution is a 1 M solution.

(T/F) The standard heat (enthalpy) of formation of graphite is zero.

(T/F) Standard heats (enthalpies) of formation of compounds, ∆H°f may be positive or negative

Select the gas with the largest root-mean- square molecular speed at 25°C. A) NH₃ B) CO C) H₂ D) SF₆ E) All the gases have the same root-mean- square molecular speed at 25°C

Calculate the root-mean- square speed of methane, CH 4 (g), at 78°C. A) 23 m/s B) 350 m/s C) 550 m/s D) 667 m/s E) 740 m/s

The air pressure in a volleyball is 75 psi. What is this pressure in torr? A) 520 torr B) 562 torr C) 3900 torr D) 7600 torr E) 75,000 torr

"The volume of an ideal gas is directly proportional to the number of moles of the gas at constant temperature and pressure" is a statement of _____________ Law. A) Charles' B) Boyle's C) Amontons' D) Avogadro's E) Dalton's

"The pressure of an ideal gas is inversely proportional to its volume at constant temperature and number of mole"; is a statement of __________________ Law. A) Charles' B) Boyle's C) Amontons' D) Avogadro's E) Gay-Lussac's

"The volume of an ideal gas is directly proportional to its absolute temperature at constant pressure and number of mole" is a statement of ________________ Law. A) Charles' B) Boyle's C) Amontons' D) Avogadro's E) Dalton's

"The total pressure in a mixture of unreacting gases is equal to the sum of the partial pressures of the individual gase" is a statement of __________________ Law. A) Charles' B) Graham's C) Boyle's D) Avogadro's E) Dalton's

"The rate of effusion of a gas is inversely proportional to the square root of its molar mass" is a statement of _________________ Law. A) Charles' B) Graham's C) Dalton's D) Avogadro's E) Boyle's

Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its pressure, other factors remaining constant? IMAGE FROM QUESTION 11(Pressure) A) a B) b C) c D) d E) e

Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its absolute temperature, other factors remaining IMAGE FROM QUESTION 12 (Temperature) A) a B) b C) c D) d E) e

Which of the lines on the figure below is the best representation of the relationship between the volume of a gas and its Celsius temperature, other factors remaining constant? IMAGE FROM QUESTION 13 (Temperature) A) a B) b C) c D) d E) e

Which of the lines on the figure below is the best representation of the relationship between the volume and the number of moles of a gas, measured at constant temperature and pressure? IMAGE FROM QUESTION 14 (n Mol) A) a B) b C) c D) d E) e

A sample of an ideal gas has its volume doubled while its temperature remains constant. If the original pressure was 100 torr, what is the new pressure? A) 10 torr B) 50 torr C) 100 torr D) 200 torr E) 1000 torr

A sample of the inert gas krypton has its pressure tripled while its temperature remained constant. If the original volume is 12 L, what is the final volume? A) 4.0 L B) 6.0 L C) 9 L D) 36 L E) 48 L

A sample of nitrogen gas at 298 K and 745 torr has a volume of 37.42 L. What volume will it occupy if the pressure is increased to 894 torr at constant temperature? A) 22.3 L B) 31.2 L C) 44.9 L D) 112 L E) 380 L

A sample of carbon dioxide gas at 125°C and 248 torr occupies a volume of 275 L. What will the gas pressure be if the volume is increased to 321 L at 125°C? A) 212 torr B) 289 torr C) 356 torr D) 441 torr E) 359 torr

A sample of oxygen gas has its absolute temperature halved while the pressure of the gas remained constant. If the initial volume is 400 mL, what is the final volume? A) 20 mL B) 133 mL C) 200 mL D) 400 mL E) 800 mL

A sample container of carbon monoxide occupies a volume of 435 mL at a pressure of 785 torr and a temperature of 298 K. What would its temperature be if the volume were changed to 265 mL at a pressure of 785 torr? A) 182 K B) 298 K C) 387 K D) 489 K E) 538 K

A 0.850-mole sample of nitrous oxide, a gas used as an anesthetic by dentists, has a volume of 20.46 L at 123°C and 1.35 atm. What would be its volume at 468°C and 1.35 atm? A) 5.38 L B) 10.9 L C) 19.0 L D) 38.3 L E) 77.9 L

A sample of ammonia gas at 65.5°C and 524 torr has a volume of 15.31 L. What is its volume when the temperature is -15.8°C and its pressure is 524 torr? A) 3.69 L B) 11.6 L C) 20.2 L D) 63.5 L E) It is not possible, since the volume would have to be negative.

A 500-mL sample of argon at 800 torr has its absolute temperature quadrupled. If the volume remains unchanged, what is the new pressure? A) 200 torr B) 400 torr C) 800 torr D) 2400 torr E) 3200 torr

A 750-mL sample of hydrogen exerts a pressure of 822 torr at 325 K. What pressure does it exert if the temperature is raised to 475 K at constant volume? A) 188 torr B) 562 torr C) 1.11 x 10³ torr D) 1.20 x 10³torr E) 1.90 x 10³ torr

What are the conditions of STP? A) 0 K and l atm B) 273.15 K and 760 torr C) 0°C and 760 atm D) 273.15°C and 760 torr E) None of these choices is correct.

A sample of propane, a component of LP gas, has a volume of 35.3 L at 315 K and 922 torr. What is its volume at STP? A) 25.2 L B) 30.6 L C) 33.6 L D) 37.1 L E) 49.2 L

Nitrogen dioxide is a red-brown gas that is responsible for the color of photochemical smog. A sample of nitrogen dioxide has a volume of 28.6 L at 45.3°C and 89.9 kPa. What is its volume at STP? A) 21.8 L B) 27.6 L C) 29.6 L D) 37.6 L E) 153 L

Calculate the temperature of an argon sample at 55.4 kPa and 18.6 L if it occupies 25.8 L at 75.0°C and 41.1 kPa. A) 95.0°C B) 85.1°C C) 77.2°C D) 72.9°C E) 65.2°C

A 250.0-mL sample of ammonia, NH 3 (g), exerts a pressure of 833 torr at 42.4°C. What mass of ammonia is in the container? A) 0.0787 g B) 0.180 g C) 8.04 g D) 17.0 g E) 59.8 g

A gas mixture consists of equal masses of methane (molecular weight 16.0) and argon (atomic weight 40.0). If the partial pressure of argon is 200. torr, what is the pressure of methane, in torr? A) 80.0 torr B) 200. torr C) 256 torr D) 500. torr E) 556 torr

Which of the following gases effuses most rapidly? A) nitrogen B) oxygen C) hydrogen chloride D) ammonia E) carbon monoxide

Which of the following gases will be the slowest to diffuse through a room? A) methane, CH₄ B) hydrogen sulfide, H₂S C) carbon dioxide, CO₂ D) water, H₂O E) neon, Ne

Arrange the following gases in order of increasing rate of effusion. C₂H₆ Ar HCl PH₃ A) Ar < HCl < PH₃ < C₂H₆ B) C₂H₆ < PH₃ < HCl < Ar C) Ar < PH₃ < C₂H₆ < HCl D) C₂H₆ < HCl < PH₃ < Ar E) Ar < PH₃< HCl < C₂H₆

(T/F) The average kinetic energy of gas molecules is proportional to the absolute temperature.

(T/F) The rate of diffusion of a gas is inversely proportional to its molar mass.

(T/F) For a gas obeying Boyle's Law, a plot of V versus 1/P will give a straight line passing through the origin.

(T/F) For a gas obeying Charles' Law, a plot of V versus 1/T will give a straight line passing through the origin.

(T/F) At a temperature of absolute zero, the volume of an ideal gas is zero.

Which of the following will be least soluble in water? A) potassium sulfate, K₂SO₄ B) ammonium nitrate, NH₄NO₃ C) chloromethane, CH₃Cl D) calcium chloride, CaCl₂ E) ethanol, C₂H₆O

Which of the following solutions will be the poorest conductor of electrical current? A) sucrose, C₁₂H₂₂O₁₁(aq) B) sodium chloride, NaCl(aq) C) potassium nitrate, KNO₃(aq) D) lithium hydroxide, LiOH(aq) E) sulfuric acid, H₂SO₄(aq)

Which of the following solutions will be the best conductor of electrical current? A) methyl alcohol, CH₃OH(aq) B) glucose, C₆H₁₂O₆(aq) C) potassium chloride, KCl(aq) D) bromine, Br₂(aq) E) ethylene glycol, C₂H₆O₂(aq)

In the following reaction, what ions, if any, are spectator ions? Pb(NO₃)₂(aq) + 2NaCl(aq) → PbCl₂(s) + 2NaNO₃(aq) A) Pb²⁺(aq), Cl⁻(aq) B) Na⁺(aq), NO₃⁻(aq) C) Pb²⁺(aq), NO₃⁻(aq) D) Na⁺(aq), Cl⁻(aq) E) There are no spectator ions.

Select the precipitate that forms when the following reactants are mixed. Na₂CO₃(aq) + BaCl₂(aq) → A) Ba₂CO₃ B) BaCO₃ C) NaCl D) NaCl₂ E) BaO

Select the precipitate that forms when the following reactants are mixed. Mg(CH₃COO)₂(aq) + LiOH(aq) → A) LiCH₃COO B) Li(CH₃COO)2 C) MgOH D) Mg(OH)₂ E) CH₃OH

Select the net ionic equation for the reaction between sodium chloride and mercury(I) nitrate. 2NaCl(aq) + Hg₂(NO₃)₂(aq) → NaNO₃(aq) + Hg₂Cl₂(s) A) Na⁺(aq) + NO₃⁻(aq) → NaNO₃(aq) B) Hg₂²⁺(aq) + 2Cl⁻(aq) → Hg₂Cl₂(s) C) NaCl(aq) → Na⁺(aq) + Cl⁻(aq) D) Hg₂(NO₃)₂(aq) → Hg₂²⁺(aq) + 2NO₃⁻(aq) E) Hg₂²⁺(aq) → Hg₂(s)

Which of the following is a weak acid? A) H₂SO₄ B) HNO₃ C) HF D) HBr E) HCl

Which of the following is a strong acid? A) H₃PO₄ B) HNO₃ C) HF D) CH₃COOH E) H₂O

Which of the following is a strong base? A) NH₃ B) Ca(OH)₂ C) Al(OH)₃ D) B(OH)₃ E) CH₃OH

Calculate the oxidation number of the chlorine in perchloric acid, HClO₄, a strong oxidizing agent. A) -1 B) +4 C) +5 D) +7 E) None of these is the correct oxidation number.

Calculate the oxidation number of sulfur in sodium metabisulfite, Na₂S₂O₅. A) -2 B) +2 C) +4 D) +5 E) None of these is the correct oxidation number.

Sodium tripolyphosphate is used in detergents to make them effective in hard water. Calculate the oxidation number of phosphorus in Na₅P₃O₁₀. A) +3 B) +5 C) +10 D) +15 E) None of these is the correct oxidation number.

Identify the oxidizing agent in the following redox reaction. Hg²⁺(aq) + Cu(s) → Cu²⁺(aq) + Hg(l) A) Hg²⁺(aq) B) Cu(s) C) Cu²⁺(aq) D) Hg(l) E) Hg²⁺(aq) and Cu²⁺(aq)

Sodium thiosulfate, Na2S2O3, is used as a "fixer" in black and white photography. Identify the reducing agent in the reaction of thiosulfate with iodine. 2S₂O₃²⁻(aq) _ I₂(aq) → S₄O₆²⁻(aq) + 2I⁻(aq) A) I₂(aq) B) I⁻(aq) C) S₂O₃²⁻(aq) D) S₄O₆²⁻(aq) E) S₂O₃²⁻(aq) and I⁻(aq)

The compound P₄O₁₀ is used in refining sugar. Select the classification for the reaction in which it is synthesized. P₄(s) + 5O₂(g) → P₄O₁₀(s) A) combination B) decomposition C) displacement D) acid-base E) precipitation

Select the classification for the following reaction. 2NaCl(l) --electricity--> 2Na(l) + Cl₂(g) A) acid-base B) precipitation C) combination D) displacement E) decomposition

Select the classification for the following reaction. CaCl₂·H₂O(s) --heat--> CaCl₂(s) + H₂O(g) A) combination B) decomposition C) displacement D) acid-base E) precipitation

Select the classification for the following reaction. 2Ag⁺(aq) + Zn(s) → 2Ag(s) + Zn²⁺(aq) A) displacement B) decomposition C) combination D) precipitation E) acid-base

Predict the product(s) for the following reaction. H₂SO₄(aq) + KOH(aq) → A) K₂SO4(aq) + H₂O(l) B) K₂S(aq) + H₂O(l) C) K(s) + H₂(g) + SO₃(g) D) KSO4(aq) + H2O(l) E) No reaction occurs.

How many moles of ions are released when 5.0 mol of cobalt(II) chloride, CoCl₂, is dissolved in water? A) 0.81 mol B) 14.4 mol C) 27 mol D) 15 mol E) 0.090 mol

How many moles of ions are released when 1 mol of ammonium phosphate, (NH₄)₃PO₄, is dissolved in water? A) 0.40 mol B) 1.6 mol C) 3.2 mol D) 4 mol E) 6.4 mol

How many moles of H+(aq) ions are present in 2500 mL of 0.65 M hydrochloric acid? A) 1.2 mol B) 0.98 mol C) 1.6 mol D) 0.65 mol E) 0.49 mol

How many moles of H+ (aq) ions are present in 4.5 L of 0.75 M nitric acid? A) 0.60 mol B) 0.75 mol C) 0.94 mol D) 3.4 mol E) 1.9 mol

How many sodium ions are present in 325 mL of 0.850 M Na₂SO₄? A) 1.66 x 10²³ Na ions B) 3.33 x 10²³ Na ions C) 4.99 x 10²³ Na ions D) 6.20 x 10²³ Na ions E) 1.57 x 10²⁴ Na ions

(T/F) In an acid-base (neutralization) reaction the equivalence point is the point where the indicator changes color.

(T/F) A particular reaction may be both a precipitation and an acid-base (neutralization) reaction.

(T/F) In a redox reaction, the reducing agent undergoes loss of electrons.

(T/F) In a redox reaction, the oxidizing agent undergoes loss of electrons.

(T/F) All combustion reactions are classified as combination reactions.