Chapter 10.2

The volume of fluorine gas required to react with 4.26 g of calcium bromide to form calcium fluoride and bromine at 25.0 °C and 4195 torr is ________ L. A) 0.0943 B) 0.241 C) 241 D) 1.24 × 10-4 E) 0.124

A) 0.0943

A gas vessel is attached to an open-end manometer filled with a nonvolatile liquid of density 0.993 g/mL as shown below. The difference in heights of the liquid in the two sides of the manometer is 32.3 mm when the atmospheric pressure is 765 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is ________ atm. A) 1.05 B) 1.01 C) 0.976 D) 0.993 E) 1.08

A) 1.05

The amount of gas that occupies 60.82 L at 31.0 °C and 367 mm Hg is ________ mol. A) 1.18 B) 0.850 C) 894 D) 11.6 E) 0.120

A) 1.18

A gas in a 325 mL container has a pressure of 695 torr at 19 °C. There are ________ mol of gas in the flask. A) 1.24 × 10-2 B) 1.48 × 10-2 C) 9.42 D) 12.4 E) 80.6

A) 1.24 × 10-2

The volume of hydrogen gas at 38.0 °C and 763 torr that can be produced by the reaction of 4.33 g of zinc with excess sulfuric acid is ________ L. A) 1.68 B) 2.71 × 10-4 C) 3.69 × 104 D) 2.84 E) 0.592

A) 1.68

CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm. A) 10.3 B) 4.02 C) 6.31 D) 0.292 E) 1.60

A) 10.3

The reaction of 50 mL of Cl2 gas with 50 mL of CH4 gas via the equation: Cl2 (g) + CH4 (g) → HCl (g) + CH3Cl (g) will produce a total of ________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 200 D) 150 E) 250

A) 100

The molecular weight of a gas that has a density of 7.10 g/L at 25.0 °C and 1.00 atm pressure is ________ g/mol. A) 174 B) 14.6 C) 28.0 D) 5.75 × 10-3 E) 6.85 × 10-2

A) 174

SO2 (5.00 g) and CO2 (5.00 g) are placed in a 750.0 mL container at 50.0 °C. The partial pressure of SO2 in the container was ________ atm. A) 2.76 B) 4.02 C) 6.78 D) 0.192 E) 1.60

A) 2.76

The molecular weight of a gas is ________ g/mol if 6.7 g of the gas occupies 6.3 L at STP. A) 24 B) 3.6 × 103 C) 27 D) 3.0 × 102 E) 1.8 × 10-2

A) 24

The pressure in a 12.2 L vessel that contains 2.34 g of carbon dioxide, 1.73 g of sulfur dioxide, and 3.33 g of argon, all at 42 °C is ________ mm Hg. A) 263 B) 134 C) 395 D) 116 E) 0.347

A) 263

What volume (L) of NH3 gas at STP is produced by the complete reaction of 7.5 g of H2O according to the following reaction? Mg3N2 (s) + 6H2O (l) → 3Mg(OH)2 (aq) + 2NH3 (g) A) 3.1 B) 9.3 C) 19 D) 28 E) 0.32

A) 3.1

CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO2 in the container was ________ atm. A) 4.02 B) 10.3 C) 1.60 D) 0.292 E) 6.31

A) 4.02

Ammonium nitrite undergoes thermal decomposition to produce only gases: NH4NO2 (s) → N2 (g) + 2H2O (g) What volume (L) of gas is produced by the decomposition of 35.0 g of NH4NO2(s) at 525 °C and 1.5 atm? A) 48 B) 160 C) 15 D) 72 E) 24

A) 48

Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 2NaN3 (s) → 2Na (s) + 3N2 (g). What mass (g) of NaN3 is required to provide 26.5 L of N2 at 22.0 °C and 1.10 atm? A) 52.2 B) 700. C) 0.807 D) 1.21 E) 1.10

A) 52.2

A gas at a pressure of 10.0 Pa exerts a force of ________ N on an area of 5.5 m2. A) 55 B) 0.55 C) 5.5 D) 1.8 E) 18

A) 55

CO (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO in the container was ________ atm. A) 6.29 B) 4.02 C) 10.3 D) 0.292 E) 1.60

A) 6.29

What volume (mL) of sulfur dioxide can be produced by the complete reaction of 3.82 g of calcium sulfite with excess HCl (aq), when the final SO2 pressure is 827 torr at 44.0 °C? A) 7.60 × 102 B) 1.39 × 10-4 C) 1.00 × 10-3 D) 0.106 E) 5.78 × 102

A) 7.60 × 102

The temperature of a sample of CH4 gas (10.34 g) in a 50.0 L vessel at 1.33 atm is ________ °C. A) 984 B) -195 C) 195 D) 1260 E) -1260

A) 984

A 0.133 mol sample of gas in a 525 mL container has a pressure of 312 torr. The temperature of the gas is ________ °C. A) 20.3 B) -253 C) -20.3 D) 203 E) 22.4

B) -253

The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is ________ g/L. A) 3.86 B) 0.719 C) 0.432 D) 0.194 E) 4.22 × 10-2

B) 0.719

A gas vessel is attached to an open-end manometer containing a nonvolatile liquid of density 0.791 g/mL as shown below. The difference in heights of the liquid in the two sides of the manometer is 43.4 cm when the atmospheric pressure is 755 mm Hg. Given that the density of mercury is 13.6 g/mL, the pressure of the enclosed gas is ________ atm. A) 1.03 B) 0.967 C) 0.993 D) 0.990 E) 0.987

B) 0.967

The amount of gas that occupies 36.52 L at 68.0 °C and 672 mm Hg is ________ mol. A) 127 B) 1.15 C) 878 D) 24.4 E) 12.7

B) 1.15

The molecular weight of a gas that has a density of 6.70 g/L at STP is ________ g/mol. A) 4.96 × 102 B) 1.50 × 102 C) 7.30 × 101 D) 3.35 E) 2.98 × 10-1

B) 1.50 × 102

The molecular weight of a gas that has a density of 5.75 g/L at STP is ________ g/mol. A) 3.90 B) 129 C) 141 D) 578 E) 1.73 × 10-3

B) 129

A sample of a gas originally at 25 °C and 1.00 atm pressure in a 2.5 L container is subject to a pressure of 0.85 atm and a temperature of 15 °C. The final volume of the gas is ________ L. A) 3.0 B) 2.8 C) 2.6 D) 2.1 E) 0.38

B) 2.8

A gas mixture of Ne and Ar has a total pressure of 4.00 atm and contains 16.0 mol of gas. If the partial pressure of Ne is 2.75 atm, how many moles of Ar are in the mixture? A) 11.0 B) 5.00 C) 6.75 D) 9.25 E) 12.0

B) 5.00

The reaction of 25 mL of N2 gas with 75 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g) will produce ________ mL of ammonia if pressure and temperature are kept constant. A) 250 B) 50 C) 200 D) 150 E) 100

B) 50

The reaction of 50 mL of Cl2 gas with 50 mL of C2H4 gas via the equation: Cl2 (g) + C2H4 (g) → C2H4Cl2 (g) will produce a total of ________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 25 D) 125 E) 150

B) 50

A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample weighing 9.49 g occupies ________ L at 353 K and 2.00 atm. A) 109 B) 68.2 C) 54.7 D) 147 E) 77.3

B) 68.2

In a Torricelli barometer, a pressure of one atmosphere supports a 760 mm column of mercury. If the original tube containing the mercury is replaced with a tube having twice the diameter of the original, the height of the mercury column at one atmosphere pressure is ________ mm. A) 380 B) 760 C) 1.52 × 103 D) 4.78 × 103 E) 121

B) 760

The pressure of a sample of CH4 gas (6.022 g) in a 30.0 L vessel at 402 K is ________ atm. A) 2.42 B) 6.62 C) 0.413 D) 12.4 E) 22.4

C) 0.413

A mixture of He and Ne at a total pressure of 0.95 atm is found to contain 0.32 mol of He and 0.56 mol of Ne. The partial pressure of Ne is ________ atm. A) 1.7 B) 1.5 C) 0.60 D) 0.35 E) 1.0

C) 0.60

A sample of a gas (5.0 mol) at 1.0 atm is expanded at constant temperature from 10 L to 15 L. The final pressure is ________ atm. A) 1.5 B) 7.5 C) 0.67 D) 3.3 E) 15

C) 0.67

Sodium hydride reacts with excess water to produce aqueous sodium hydroxide and hydrogen gas: NaH (s) + H2O (l) → NaOH (aq) + H2 (g) A sample of NaH weighing ________ g will produce 982 mL of gas at 28.0 °C and 765 torr, when the hydrogen is collected over water. The vapor pressure of water at this temperature is 28 torr. A) 2.93 B) 0.960 C) 0.925 D) 0.0388 E) 925

C) 0.925

A sample of a gas originally at 29 °C and 1.25 atm pressure in a 3.0 L container is allowed to contract until the volume is 2.2 L and the temperature is 11 °C. The final pressure of the gas is ________ atm. A) 2.9 B) 2.8 C) 1.6 D) 2.1 E) 0.38

C) 1.6

The density of chlorine (Cl2) gas at 25 °C and 60. kPa is ________ g/L. A) 20 B) 4.9 C) 1.7 D) 0.86 E) 0.58

C) 1.7

The mass of nitrogen dioxide contained in a 4.32 L vessel at 48 °C and 141600 Pa is ________ g. A) 5.35 × 104 B) 53.5 C) 10.5 D) 70.5 E) 9.46 × 10-2

C) 10.5

The volume of HCl gas required to react with excess magnesium metal to produce 6.82 L of hydrogen gas at 2.19 atm and 35.0 °C is ________ L. A) 6.82 B) 2.19 C) 13.6 D) 4.38 E) 3.41

C) 13.6

The thermal decomposition of potassium chlorate can be used to produce oxygen in the laboratory. 2KClO3 (s) → 2KCl (s) + 3O2 (g) What volume (L) of O2 gas at 25 °C and 1.00 atm pressure is produced by the decomposition of 7.5 g of KClO3 (s)? A) 4.5 B) 7.5 C) 2.3 D) 3.7 E) 11

C) 2.3

A gas at a pressure of 325 torr exerts a force of ________ N on an area of 5.5 m2. A) 1.8 × 103 B) 59 C) 2.4 × 105 D) 0.018 E) 2.4

C) 2.4 × 105

The reaction of 100 mL of Cl2 gas with 100 mL of CH4 gas via the equation: Cl2 (g) + CH4 (g) → HCl (g) + CH3Cl (g) will produce a total of ________ mL of products if pressure and temperature are kept constant. A) 100 B) 50 C) 200 D) 150 E) 250

C) 200

The Mond process produces pure nickel metal via the thermal decomposition of nickel tetracarbonyl: Ni(CO)4 (l) → Ni (s) + 4CO (g). What volume (L) of CO is formed from the complete decomposition of 444 g of Ni(CO)4 at 752 torr and 22.0 °C? A) 0.356 B) 63.7 C) 255 D) 20.2 E) 11.0

C) 255

The molecular weight of a gas is ________ g/mol if 3.5 g of the gas occupies 2.1 L at STP. A) 41 B) 5.5 × 103 C) 37 D) 4.6 × 102 E) 2.7 × 10-2

C) 37

The root-mean-square speed of CO at 113 °C is ________ m/s. A) 317 B) 58.3 C) 586 D) 993 E) 31.5

C) 586

A sample of He gas (2.0 mmol) effused through a pinhole in 53 s. The same amount of an unknown gas, under the same conditions, effused through the pinhole in 248 s. The molecular mass of the unknown gas is ________ g/mol. A) 0.19 B) 5.5 C) 88 D) 19 E) 350

C) 88

In a gas mixture of He, Ne, and Ar with a total pressure of 8.40 atm, the mole fraction of Ar is ________ if the partial pressures of He and Ne are 1.50 and 2.00 atm, respectively. A) 0.179 B) 0.238 C) 0.357 D) 0.583 E) 0.417

D) 0.583

A flask contains a mixture of He and Ne at a total pressure of 2.6 atm. There are 2.0 mol of He and 5.0 mol of Ne in the flask. The partial pressure of He is ________ atm. A) 9.1 B) 6.5 C) 1.04 D) 0.74 E) 1.86

D) 0.74

A sample of a gas (1.50 mol) is contained in a 15.0 L cylinder. The temperature is increased from 100 °C to 150 °C. The ratio of final pressure to initial pressure [p2/p1 ] is ________. A) 1.50 B) 0.667 C) 0.882 D) 1.13 E) 1.00

D) 1.13

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.00 mol of neon gas at is ________ atm. (a = 0.211 L2-atm/mol2, b = 0.0171 L/mol) A) 0.730 B) 1.00 C) 1.21 D) 1.37 E) 0.367

D) 1.37

A sample of H2 gas (2.0 L) at 3.5 atm was combined with 1.5 L of N2 gas at 2.6 atm pressure at a constant temperature of 25 °C into a 7.0 L flask. The total pressure in the flask is ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C. A) 0.56 B) 2.8 C) 1.0 D) 1.6 E) 24

D) 1.6

The volume of hydrogen gas at 45.0 °C and 699 torr that can be produced by the reaction of 5.66 g of zinc with excess sulfuric acid is ________ L. A) 2.84 B) 2.71 × 10-4 C) 3.69 × 104 D) 2.45 E) 0.592

D) 2.45

A vessel contained N2, Ar, He, and Ne. The total pressure in the vessel was 987 torr. The partial pressures of nitrogen, argon, and helium were 44.0, 486, and 218 torr, respectively. The partial pressure of neon in the vessel was ________ torr. A) 42.4 B) 521 C) 19.4 D) 239 E) 760

D) 239

If 50.75 g of a gas occupies 10.0 L at STP, 129.3 g of the gas will occupy ________ L at STP. A) 3.92 B) 50.8 C) 12.9 D) 25.5 E) 5.08

D) 25.5

A sample of He gas (3.0 L) at 5.6 atm and 25 °C was combined with 4.5 L of Ne gas at 3.6 atm and 25 °C at constant temperature in a 9.0 L flask. The total pressure in the flask was ________ atm. Assume the initial pressure in the flask was 0.00 atm and the temperature upon mixing was 25 °C. A) 2.6 B) 9.2 C) 1.0 D) 3.7 E) 24

D) 3.7

A sample of N2 gas (2.0 mmol) effused through a pinhole in 5.5 s. It will take ________ s for the same amount of CH4 to effuse under the same conditions. A) 7.3 B) 5.5 C) 3.1 D) 4.2 E) 9.6

D) 4.2

A sample of O2 gas (2.0 mmol) effused through a pinhole in 5.0 s. It will take ________ s for the same amount of CO2 to effuse under the same conditions. A) 4.3 B) 0.23 C) 3.6 D) 5.9 E) 6.9

D) 5.9

SO2 (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The total pressure in the container was ________ atm. A) 0.192 B) 4.02 C) 2.76 D) 6.78 E) 1.60

D) 6.78

Automobile air bags use the decomposition of sodium azide as their source of gas for rapid inflation: 2NaN3 (s) → 2Na (s) + 3N2 (g). What mass (g) of NaN3 is required to provide 40.0 L of N2 at 25.0 °C and 763 torr? A) 1.64 B) 1.09 C) 160 D) 71.1 E) 107

D) 71.1

The volume of fluorine gas required to react with 2.67 g of calcium bromide to form calcium fluoride and bromine at 41.0 °C and 4.31 atm is ________ mL. A) 10.4 B) 210 C) 420 D) 79.9 E) 104

D) 79.9

The volume of 0.25 mol of a gas at 72.7 kPa and 15 °C is ________ m3. A) 8.1 × 10-5 B) 1.2 × 10-4 C) 4.3 × 10-4 D) 8.2 × 10-3 E) 2.2 × 10-1

D) 8.2 × 10-3

Using the van der Waals equation, the pressure in a 22.4 L vessel containing 1.50 mol of chlorine gas at 0.00 °C is ________ atm. (a = 6.49 L2-atm/mol2, b = 0.0562 L/mol) A) 0.993 B) 1.50 C) 0.676 D) 1.91 E) 1.48

E) 1.48

The reaction of 50 mL of N2 gas with 150 mL of H2 gas to form ammonia via the equation: N2 (g) + 3H2 (g) → 2NH3 (g) will produce ________ mL of ammonia if pressure and temperature are kept constant. A) 250 B) 50 C) 200 D) 150 E) 100

E) 100

The density of N2O at 1.53 atm and 45.2 °C is ________ g/L. A) 18.2 B) 1.76 C) 0.388 D) 9.99 E) 2.58

E) 2.58

Since air is a mixture, it does not have a "molar mass." However, for calculation purposes, it is possible to speak of its "effective molar mass." (An effective molar mass is a weighted average of the molar masses of a mixture's components.) If air at STP has a density of 1.285 g/L, its effective molar mass is ________ g/mol. A) 26.94 B) 31.49 C) 30.00 D) 34.42 E) 28.80

E) 28.80

SO2 (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0 °C. The partial pressure of CO2 in the container was ________ atm. A) 6.78 B) 2.76 C) 1.60 D) 0.192 E) 4.02

E) 4.02

A gas mixture of N2 and CO2 has a total pressure of 8.00 atm and contains 12.5 mol of gas. If the partial pressure of N2 is 3.69 atm, how many moles of CO2 are in the mixture? A) 5.77 B) 3.69 C) 4.31 D) 11.0 E) 6.73

E) 6.73