Chapter 10.3
Of the following gases, ________ has density of 0.906 g/L at 315 K and 1.16 atm. A) Ne B) Ar C) Kr D) Xe E) He
A) Ne
Given the equation: C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced) Determine the number of liters of O2 consumed at STP when 60.0 grams of C2H6 is burned.
157
Given the equation: C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced) Determine the number of liters of CO2 formed at STP when 270.0 grams of C2H6 is burned in excess
403
A 0.325 L flask filled with gas at 0.851 atm and 19 °C contains ________ mol of gas. A) 0.0116 B) 0.0148 C) 9.42 D) 12.4 E) 80.7
A) 0.0116
A mixture of Xe, Kr, and Ar has a total pressure of 6.69 atm. What is the mole fraction of Kr if the partial pressures of Xe and Ar are 1.92 atm and 2.75 atm, respectively. A) 0.302 B) 0.287 C) 0.411 D) 0.259 E) 0.698
A) 0.302
A vessel containing Ne(g) and Ar(g) has a total pressure of 9.78. If the partial pressure of the Neon (PNe) is 3.78 and the partial pressure of the Argon (PAr) is 6, then the mole-fraction of Ne(g) is _______ and the mole-fraction of Ar(g) is ________. A) 0.39, 0.61 B) 0.61, 0.39 C) 37, 58.7 D) 0.63, 1.59 E) 2.59, 1.63
A) 0.39, 0.61
Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) In an experiment, 177 mL of wet H2 is collected over water at 27 °C and a barometric pressure of 766 torr. The vapor pressure of water at 27 °C is 26.74 torr. The partial pressure of hydrogen in this experiment is ________ atm. A) 0.972 B) 739 C) 1.01 D) 793 E) 1.04
A) 0.972
A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 751 torr. Use Boyle's law to calculate the pressure (torr) when the volume is reduced to 7.25 L at a constant temperature of 25.0 °C. A) 1.04 × 103 B) 0.097 C) 5.44 × 104 D) 544 E) 1.36
A) 1.04 × 103
How many moles of gas are there in a 36.3 L container at 25.2 °C and 570.3 mm Hg? A) 1.11 B) 13.2 C) 0.863 D) 0.0110 E) 16,700
A) 1.11
The density of HCN is ________ g/L at STP. A) 1.21 B) 329 C) 605 D) 0.829 E) 2.21
A) 1.21
The density of NO2 in a 4.77 L tank at 738.4 torr and 45.0 °C is ________ g/L. A) 1.71 B) 1300 C) 12.1 D) 0.0169 E) 8.17
A) 1.71
30.0 grams of argon and 15.0 grams of xenon are placed in a 170.9 ml container at 21.8 °C. The partial pressure of xenon is ________ atm. A) 16.1 B) 106 C) 1.20 D) 0.472 E) 228
A) 16.1
10.0 grams of argon and 20.0 grams of neon are placed in a 1216.1 ml container at 25.1 °C. The partial pressure of neon is ________ atm. A) 19.9 B) 5.03 C) 1.68 D) 20.0 E) 49.1
A) 19.9
The density (in g/L) of CO2 at 1106.2 torr and 56.3 °C is ________. A) 2.37 B) 1800 C) 13.9 D) 0.0234 E) 0.0538
A) 2.37
How many moles of gas are there in a 53.7 L container at 24.6 °C and 845.9 torr? A) 2.45 B) 29.6 C) 0.409 D) 0.0241 E) 1860
A) 2.45
A vessel contains a mixture of 34.9 grams of H2 (g) and 17.7 grams of CH4. If the total pressure inside the vessel is measured at 2.92 atm, the partial pressure of H2 (g) must be _____ atm. A) 2.75 B) 50.5 C) 0.175 D) 53.8 E) 5.53
A) 2.75
A helium balloon is filled to a volume of 27.7 L at 300 K. What will the volume of the balloon become if the balloon is heated to raise the temperature to 392 K? A) 36.2 B) 21.2 C) 0.0276 D) 0.0472 E) 3,260,000
A) 36.2
The root-mean-square speed of NO2 at 28.4 °C is ________ m/sec. A) 404 B) 40.2 C) 124 D) 233 E) 12.8
A) 404
The volume of 1.26 mol of gas at 69.4 kPa and 25.30 °C is ________ L. A) 45.1 B) 633 C) 3.82 D) 0.445 E) 0.439
A) 45.1
The root-mean-square speed of N2 at 33.5 °C is ________ m/sec. A) 522 B) 51.9 C) 173 D) 302 E) 16.5
A) 522
A closed-end manometer was attached to a vessel containing argon. The difference in the mercury levels in the two arms of the manometer was 9.60 cm. Atmospheric pressure was 783 mm Hg. The pressure of the argon in the container was ________ mm Hg. A) 96.0 B) 661 C) 773 D) 793 E) 882
A) 96.0
The density of ________ is 1.70 g/L at STP. A) F2 B) NO C) CH4 D) Ne E) CO
A) F2
Molecular compounds of low molecular weight tend to be gases at room temperature. Which of the following is most likely not a gas at room temperature? A) KBr B) F2 C) HCN D) SO2 E) CH4
A) KBr
According to kinetic-molecular theory, in which of the following gases will the root-mean-square speed of the molecules be the highest at 200 °C? A) NH3 B) N2O C) O2 D) UF6 E) None. The molecules of all gases have the same root-mean-square speed at any given temperature.
A) NH3
Zinc reacts with aqueous sulfuric acid to form hydrogen gas: Zn (s) + H2SO4 (aq) → Zn SO4 (aq) + H2 (g) In an experiment, 201 mL of wet H2 is collected over water at 27 °C and a barometric pressure of 765 torr. How many grams of Zn have been consumed? The vapor pressure of water at 27 °C is 26.74 torr. A) 4.38 × 106 B) 0.519 C) 519 D) 394 E) 3.94 × 105
B) 0.519
A fixed amount of gas at 25.0 °C occupies a volume of 8.66 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 112 °C while maintaining the pressure at 629 torr. A) 9.26 B) 11.2 C) 1.93 D) 6.70 E) 38.8
B) 11.2
A sample of an ideal gas (3.00 L) in a closed container at 25.0 °C and 76.0 torr is heated to 270 °C. The pressure of the gas at this temperature is ________ torr. A) 912 B) 138 C) 76.5 D) 39.5 E) 0.0253
B) 138
A balloon originally had a volume of 4.39 L at 44 °C and a pressure of 729 torr. The balloon must be cooled to ________ °C to reduce its volume to 3.99 L (at constant pressure). A) 0.00 B) 15.1 C) -288 D) 288 E) 546
B) 15.1
The pressure exerted by 1.0 mol of gas in a 13 L flask at 22 °C is ________ kPa. A) 560 B) 190 C) 18 D) 2.4 E) 1.0
B) 190
A sample of gas (1.9 mol) is in a flask at 21 °C and 697 mm Hg. The flask is opened and more gas is added to the flask. The new pressure is 841 mm Hg and the temperature is now 26 °C. There are now ________ mol of gas in the flask. A) 1.6 B) 2.3 C) 2.9 D) 3.5 E) 0.28
B) 2.3
The volume occupied by 2.3 mol of gas at 35 °C and 2.0 atm pressure is ________ L. A) 38 B) 29 C) 3.3 D) 0.053 E) 0.026
B) 29
A gas originally at 27 °C and 1.00 atm pressure in a 3.3 L flask is cooled at constant pressure until the temperature is 11 °C. The new volume of the gas is ________ L. A) 0.27 B) 3.1 C) 3.3 D) 3.5 E) 0.24
B) 3.1
The density of nitric oxide (NO) gas at 0.970 atm and 34.9 °C is ________ g/L. A) 0.0384 B) 0.869 C) 1.15 D) 0.339 E) 10.2
C) 1.15
A pressure of 0.500 atm is the same as a pressure of ________ of mm Hg. A) 193 B) 760. C) 380. D) 29.9 E) 33.0
C) 380.
A sample of gas (1.3 mol) occupies ________ L at 22 °C and 3.5 atm. A) 0.079 B) 0.67 C) 9.0 D) 14 E) 0.032
C) 9.0
A sample of He gas (2.35 mol) occupies 57.9 L at 300.0 K and 1.00 atm. The volume of this sample is ________ L at 469 K and 1.00 atm. A) 0.709 B) 41.1 C) 90.5 D) 1.41 E) 57.9
C) 90.5
A 0.333-g sample of an unknown pure gas occupies a volume of 0.255 L at a pressure of 1.00 atm and a temperature of 100.0 °C. The unknown gas is ________. A) xenon B) neon C) krypton D) helium E) argon
E) argon
The density of krypton gas at 0.866 atm and 44.4 °C is ________ g/L. A) 0.0332 B) 0.359 C) 0.238 D) 2.78 E) 5.57
D) 2.78
The volume of 0.43 mol of an ideal gas at 365 torr and 97 °C is ________ L. A) 0.054 B) 7.1 C) 11 D) 27 E) 0.024
D) 27
Calcium hydride (CaH2) reacts with water to form hydrogen gas: CaH2 (s) + 2H2O (l) → Ca(OH)2 (aq) + 2H2 (g) How many grams of CaH2 are needed to generate 48.0 L of H2 gas at a pressure of 0.995 atm and a temperature of 32 °C? A) 56.8 B) 0.954 C) 161 D) 40.1 E) 80.3
D) 40.1
If 3.21 mol of a gas occupies 56.2 L at 44 °C and 793 torr, 4.73 mol of this gas occupies ________ L under these conditions. A) 14.7 B) 61.7 C) 30.9 D) 82.8 E) 478
D) 82.8
A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L at constant temperature. After the compression, the gas pressure was ________ atm. A) 4.00 B) 2.00 C) 1.00 D) 8.00 E) 16.0
E) 16.0
The density of chlorine gas at 1.01 atm and 54.1 °C is ________ g/L. A) 0.0376 B) 0.375 C) 0.228 D) 1.33 E) 2.67
E) 2.67
At a temperature of ________ °C, 0.444 mol of CO gas occupies 11.8 L at 839 torr. A) 379 B) 73.0 C) 14.0 D) 32.0 E) 83.5
E) 83.5