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## 14.4 mL 156 mL 144 mL 865 mL 780 mL

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**The volume of a sample of a gas is 415 mL at 10.0 atm and**337 K. What volume will it occupy at 5.32 atm and 337 K? • 14.4 mL • 156 mL • 144 mL • 865 mL • 780 mL**The Rankine temperature scale is an absolute temperature**scale based on the Fahrenheit degree rather than the Celsius degree. What number (nearest whole number) goes into the blank in the formula below that allows one to convert directly from degrees Fahrenheit to degrees Rankine? °R = °F + (______)° • 273 • -273 • 470 • 460 • - 460**Choose the response that includes all of the following**statements that are correct, and no incorrect statements. Assume constant pressure in each case. If a sample of gas is I. heated from 100°C to 200°C the volume will double. II. heated from 0°C to 273°C the volume will double. III. cooled from 400°C to 200°C the volume will decrease by a factor of two. IV. cooled from 1000°C to 200°C the volume will decrease by a factor of five. V. heated from 200°C to 2000°C the volume will increase by a factor of ten. • II • I and II • III and IV • II and III • none of these**The volume of a sample of a gas is 405 mL at 10.0 atm and**467 K. What volume will the sample occupy at 10.0 atm and 1025 K? • 644 mL • 889 mL • 405 mL • 434 mL • 185 mL**A gas sample has a volume of 6.30 L at STP. What would be**its pressure if it occupied 5.70 L at 0.0°C? • 688 torr • 7.13 torr • 840. torr • 1.51 atm • 0.475 torr**Which possible response includes all the following**statements that are correct, and no incorrect statements? I. For a sample of gas held at constant pressure, a plot of volume versus temperature is a straight line. II. For a sample of gas held at constant pressure, a plot of volume versus temperature is one branch of a hyperbola. III. For a sample of gas held at constant temperature, a plot of volume versus pressure is a straight line. IV. For a sample of gas held at constant temperature, a plot of volume versus pressure is one branch of a hyperbola. V. At constant pressure the volume occupied by a definite mass of a gas varies inversely with the absolute temperature. VI. At constant pressure the volume occupied by a definite mass of a gas varies directly with the absolute temperature. VII. At constant temperature the volume occupied by a definite mass of a gas varies inversely with the applied pressure. VIII. At constant temperature the volume occupied by a definite mass of a gas varies directly with the applied pressure. • I, III, V, and VII • II, IV, VI, and VIII • I, IV, VI, and VII • II, III, V, and VIII • none of these**A sample of gas has a volume of 180. mL at -30.°C and 1.05**atm. What will be its volume at 35°C and 0.525 atm? • 52 mL • 280. mL • 456 mL • 42 mL • 114 mL**If 1.00 L of a gas is 4.40 times as heavy as 1.00 L of O2 at**the same temperature and pressure, then the molecular weight of the gaseous substance is _______. • 50.0 amu • 67.0 amu • 70.4 amu • 88.0 amu • 141 amu**What is the volume occupied by 3.50 grams of Cl2 gas at**45°C and 745 torr? • 1.17 L • 0.961 L • 1.05 L • 1.46 L • none of these**How many moles of an ideal gas are contained in 8.21 L at**73°C and 380 torr? • 0.250 • 1.5 x 1023 • 0.144 • 7.5 x 1023 • 4.2 x 10-25**A gaseous compound is 23.79% C, 5.99% H and 70.22% Cl by**mass. At STP 258 mL of the gas weighs 0.581 g. What is the molecular formula for this compound? • CH3Cl2 • CH3Cl • CH2Cl2 • C2HCl • C2H7Cl2**What is the pressure exerted by 26.0 g SO2, 4.0 g H2, and**20.2 g Ne in a 10.0-liter container at 50.0°C? • 9.04 atm • 10.1 atm • 14.4 atm • 18.6 atm • 26.3 atm**A mixture of 16.0 g of O2, 21.0 g of N2, and 16.0 g of He at**20.°C is in a 25.0-L container. What are the partial pressures of O2, N2, and He in this mixture? O2 / N2 / He • 0.481 atm / 1.44 atm / 3.85 atm • 0.481 atm / 0.721 atm / 3.85 atm • 0.962 atm / 1.44 atm / 3.85 atm • 0.481 atm / 0.721 atm / 0.240 atm • 0.962 atm / 0.721 atm / 0.240 atm**What volume of H2 at STP would be required to react**completely with 12.4 grams of Fe3O4 according to the equation below? Fe3O4(s) + 4H2(g) {image} 3Fe(s) + 4H2O(g) • 4.80 L • 16.7 L • 32.0 L • 20.4 L • 1.20 L**A 0.720-gram sample, known to contain only CaCO3 and BaCO3,**was heated until the carbonates were decomposed to oxides as indicated. After heating, the mass of the solid residue was 0.516 gram. What mass of BaCO3 was present in the sample? CaCO3(s) {image} CaO(s) + CO2(g) BaCO3(s) {image} BaO(s) + CO2(g) • 0.316 g • 0.384 g • 0.516 g • 0.463 g • 0.521 g**Which response includes all the following statements that**describe correctly the properties of gases, and no others? I. At constant temperature, the pressure increases as the volume of a definite mass of a gas increases. II. At constant pressure, the volume of a definite mass of a gas increases as the temperature increases. III. At reasonable temperatures and pressures, gases consist mostly of empty space. IV. Heating a sample of gas forces the particles closer together when the pressure and volume remain constant. V. The forces of attraction between individual gaseous particles are relatively weak. • II, III, and V • I, II, and V • III and V • II, IV, and V • I, III, and V**Calculate the ratio of the rate of effusion of CO2 to He.**• 0.090/1 • 0.30/1 • 3.3/1 • 11/1 • 12/1**A gas of unknown composition effuses at the rate of 10 mL/s**in an effusion apparatus in which CH4 gas effuses at the rate of 20 mL/s. What is the approximate molecular weight of the unknown gas? • 4 amu • 8 amu • 16 amu • 32 amu • 64 amu**Which one of the responses includes all of the following**statements that are correct, and no incorrect statements? I. At a given temperature and pressure, say 500°C and 1 atmosphere, the attractive forces between water molecules are greater than the attractive forces between ammonia molecules. II. At 500°C and 1 atmosphere pressure, the attractive forces between ammonia molecules are greater than those between water molecules. III. By elastic collisions between molecules of a gas, we refer to collisions in which there is no net gain or loss of energy. IV. If the pressure on a sample of an ideal gas is doubled while the absolute temperature is doubled, the final volume will be unchanged. V. If the pressure on a sample of an ideal gas is halved while the absolute temperature is halved, the final volume will be unchanged. • I, II, and III • III, IV, and V • I, III, IV, and V • I, IV, and V • II and IV