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30 Cards in this Set
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Which of the following statements is correct concerning the gas phase? When pressure is applied to a gas, its volume increases. Depending on their chemical nature, two or more gases can form either a homogeneous or heterogeneous mixture. The volume of a gas is always less than the volume of its container. A gas expands spontaneously to fill its container. |
A gas expands spontaneously to fill its container. |
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What pressure in units of torr is equal to 1.14 atm of pressure? 0.00150 torr; 116 torr; 1.16 torr; 866 torr |
866 torr |
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What happens to the height of the mercury column, if the atmospheric pressure increases? the height of the mercury column decreases. the height of the mercury column remains the same. the height of the mercury column increases. |
the height of the mercury column increases. |
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A gas, behaving ideally, has a pressure P1 and at a volume V1. The pressure of the gas is changed to P2. Using Avogadro’s, Charles’, or Boyle’s law, develop an expression that would solve for the new volume V2. P1/T1 = P2/T2 P1V1 = P2V2 V1/T1 = V2/T2 P1T1 = P2T2 |
P1V1 = P2V2 |
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A gas, behaving ideally, fills a fixed volume container at a pressure P1 and at a temperature T1. The temperature of the container is changed to T2. Using Avogadro’s, Charles’, or Boyle’s law, develop an expression that would solve for the new pressure P2. P1T1 = P2T2 P1/T1 = P2/T2 V1/T1 = V2/T2 P1V1 = P2V2 |
P1/T1 = P2/T2 |
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Which is a statement of Boyle's law?Which is a statement of Boyle's law? The volume of a fixed quantity of gas maintained at constant temperature is directly proportional to the pressure. The volume of a fixed quantity of gas maintained at constant temperature is inversely proportional to the pressure. The volume of a gas maintained at constant temperature and pressure is directly proportional to the number of moles of the gas. The volume of a fixed quantity of gas maintained at constant pressure is directly proportional to its absolute temperature. |
The volume of a fixed quantity of gas maintained at constant temperature is inversely proportional to the pressure. |
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Which gas deviates most from ideal behavior? |
Cl2 (lowest molar volume in L) |
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What volume is occupied by one mole of gas at STP? 0.08206 L; 22.4 mL; 22.4 L; 4.00 g |
22.4 L |
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What is the mass, in grams, of CH4 gas in a 5.00 L cylinder at a pressure of 781 torr and a temperature of 25.0 °C? 3.37 g 40.3 g 2.56 × 102 g 0.210 g |
3.37 g (HINT: The ideal gas law is expressed as PV = nRT; where P is pressure, V is volume, n is the moles of gas, R is the ideal gas constant, and T is the Kelvin temperature.) |
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Is water vapor more or less dense than under the same conditions of temperature and pressure? Water vapor is more dense than N2. Water vapor is less dense than N2. Their densities are equal. |
Water vapor is less dense than N2 |
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How many liters of CO2 gas can be produced at 30.0 °C and 1.50 atm from the reaction of 5.00 mol of C3H8 and an excess of O2 according to the following equation? C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) 27.6 L; 249 L; 24.6 L; 82.9 L |
249 L |
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How is the partial pressure exerted by N2 gas affected when some O2 is introduced into a container if the temperature and volume remain constant? The partial pressure of N2 will increase. The partial pressure of N2 will decrease. The partial pressure of N2 will not change. |
The partial pressure of N2 will not change. |
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look @ last question: How is the total pressure affected? The total pressure will increase. The total pressure will decrease. The total pressure will not change. |
The total pressure will increase. |
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What is the total pressure (in atm) inside of a vessel containing N2 exerting a partial pressure of 0.256 atm, He exerting a partial pressure of 203 mmHg, and H2 exerting a partial pressure of 39.0 kPa? 0.908 atm 1.54 × 105 atm 3.95 × 103 atm 242 atm |
0.908 atm |
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Estimate the fraction of molecules at 100 ∘C with speeds less than 300 m/s. about a third. about a quarter. about one-sixth. about a half. |
about one-sixth (on graph) |
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Consider three gases all at 298 K: HCl, H2, and O2. List the gases in order of increasing average speed |
HCl, O2, H2 |
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Which statement is consistent with the kinetic-molecular theory? The volume of a vessel containing a gas consists mainly of empty space. Gas molecules have high attractive forces between them. The average kinetic energy of gas molecules is inversely proportional to the absolute temperature. Gas molecules have discrete, directional motion. |
The volume of a vessel containing a gas consists mainly of empty space. |
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What is the ratio of urms to ump for a sample of O2(g) at 300 K? |
Urms/Ump = 1.22 |
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Will this ratio change as the temperature changes? Yes, this ratio will increase as the temperature rises. Yes, this ratio will decrease as the temperature rises. No, this ratio will not change. |
No, this ratio will not change. |
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Will it be different for a different gas? Yes, the ratio is different for each gas. Yes, the ratio depends on the number of atoms the molecule consists of. No, the ratio is the same for all gases. |
No, the ratio is the same for all gases. |
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Will these changes increase, decrease, or have no effect on the mean free path of the molecules in a gas sample? increasing pressure It will increase the mean free path of the molecules in a gas sample. It will decrease the mean free path of the molecules in a gas sample. It will have no effect on the mean free path of the molecules in a gas sample. |
It will decrease the mean free path of the molecules in a gas sample. |
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Will these changes increase, decrease, or have no effect on the mean free path of the molecules in a gas sample? increasing temperature. It will increase the mean free path of the molecules in a gas sample. It will decrease the mean free path of the molecules in a gas sample. It will have no effect on the mean free path of the molecules in a gas sample. |
It will have no effect on the mean free path of the molecules in a gas sample. |
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Which of the following correctly lists the gases in order of increasing rate of effusion? Cl2 < Ar < CH4 < He CH4 < He < Cl2 < Ar He < Ar < Cl2 < CH4 He < CH4 < Ar < Cl2 |
Cl2 < Ar < CH4 < He |
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Under which conditions do you expect helium gas to deviate most from ideal behavior? 100 K and 5 atm; 100 K and 1 atm; 300 K and 2 atm |
100 K and 5 atm |
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The Dutch scientist Johannes van der Waals developed a useful equation to predict the behavior of real gases. In the van der Waals equation, what are the constants a and b, respectively? a is a measure of the molecular mass of the gas molecules, and b is a measure of the finite volume occupied by the molecules. a is a measure of how strongly the gas molecules attract one another, and b is a measure of the finite volume occupied by the molecules. a is a measure of the finite volume occupied by the molecules, and b is a measure of how strongly the gas molecules attract one another. a is a measure of the random motion of gas molecules, and b is a measure of the volume of the container. |
a is a measure of how strongly the gas molecules attract one another, and b is a measure of the finite volume occupied by the molecules. |
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Charles's law states that the volume (V) of a fixed quantity of gas is directly proportional to its temperature (T) at a constant pressure. |
Charles's law states that the volume (V) of a fixed quantity of gas is directly proportional to its temperature (T) at a constant pressure. |
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Calculate the volume of the gas when the pressure of the gas is 1.70 atm at a temperature of 298 K. There are 160. mol of gas in the cylinder. The value for the universal gas constant R is 0.08206 L⋅atm/(mol⋅K) . |
volume = 2302 L (PV=nRT, and thus V=nRT/P.The volume of the gas is calculated by substituting the values of n, R, T, and P:V=160.mol×0.08206 L⋅atm/(mol⋅K)×298 K1.70atm=2302L) |
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In the simulation, set the temperature of the sample gas to 304 K. Click on the "Run" button and observe how the number of moles of the gas varies with an increase in the gas’s volume. Then, click on the "Reset" button, set the temperature of the sample gas to 504 K, and click on the "Run" button again.Observe the graph produced in the simulation and select the correct options listed below.Check all that apply. The volume of the sample gas increases linearly with the number of moles. Volume is inversely proportional to the number of moles of the gas. The pressure of the sample gas increases with an increase in volume. The volume of t |
The volume of the sample gas increases linearly with the number of moles. AND The volume of the gas doubles when the number of moles of the gas is doubled at the same temperature. (Thus V = kn, where, k is a proportionality constant.) |
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Imagine that the gas shown in the simulation is an ideal gas such as helium. Notice that the final number of moles of gas is 1.00 mol for each experimental run. You can find the final volume of the gas using the y axis of the graph shown.Consider an experimental run at 273 K where the initial number of moles (n1) is actually 1.00 mol, and the final number of moles (n2) is 2.00 mol. Use the simulation to find the volume (V1) of 1.00 mol of helium at 273 K and calculate the final volume (V2). |
44.8 L |
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At 4.00 L, an expandable vessel contains 0.864 mol of oxygen gas. How many liters of oxygen gas must be added at constant temperature and pressure if you need a total of 1.84 mol of oxygen gas in the vessel? |
volume that must be added = 4.52 L |
