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A sample of neon effuses from a container in 76 seconds. The same amount of an unknown noble gas requires 155 seconds. Identify the gas. 

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Calculate the ratio of effusion rates for Ar and Kr. 

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Calculate the root mean square velocity and kinetic energy of CO, CO2, and SO3 at 298 K. Which gas has the greatest velocity? The greatest kinetic energy? The greatest effusion rate? 

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A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon.

d. If a small hole were opened in the flask, which gas would effuse more quickly? 

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A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon.

c. The molecules of which gas have the greater average kinetic energy?

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A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon.

b. The molecules or atoms of which gas have the greater average velocity?

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A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon.

a. Which of the two gases exerts the greater partial pressure?

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Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. 

d. Which gas sample would have the faster rate of effusion? 

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Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. 

 Do the argon atoms, because they are more massive, exert a greater pressure on the walls of the container? Explain. 

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Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. 

b. Do the atoms in the helium sample have the same average velocity as the atoms in the argon sample? 

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Consider a 1.0-L sample of helium gas and a 1.0-L sample of argon gas, both at room temperature and atmospheric pressure. 

a. Do the atoms in the helium sample have the same average kinetic energy as the atoms in the argon sample? 

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Hydrogen gas (a potential future fuel) can be formed by the reaction of methane with water according to the equation: 

CH4(g) + H2O(g) → CO(g) + 3 H2(g)

In a particular reaction, 25.5 L of methane gas (measured at a pressure of 732 torr and a temperature of 25 °C) mixes with 22.8 L of water vapor (measured at a pressure of 702 torr and a temperature of 125 °C). The reaction produces 26.2 L of hydrogen gas at STP. What is the percent yield of the reaction?

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Lithium reacts with nitrogen gas according to the reaction: 

6 Li(s) + N2(g) → 2 Li3N(s)

What mass of lithium (in g) reacts completely with 58.5 mL of N2 gas at STP?

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Automobile air bags inflate following a serious impact. The impact triggers the chemical reaction: 

2 NaN3(s) →  2Na(s) + 3 N2(g)

If an automobile air bag has a volume of 11.8 L, what mass of NaN 3 (in g) is required to fully inflate the air bag upon impact? Assume STP conditions. 

 

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Oxygen gas reacts with powdered aluminum according to the reaction: 

4 Al(s) + 3 O2(g) → 2 Al2O3(s)

What volume of O2 gas (in L), measured at 782 mmHg and 25 °C, completely reacts with 53.2 g AI?

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CH3OH can be synthesized by the reaction: 

CO(g) + 2 H2(g) → CH3OH

What volume of H2 gas (in L), at 748 mmHg and 86 °C, is required to synthesize 25.8 g CH 3OH? How many liters of CO gas, measured under the same conditions, is required? 

 

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Consider the chemical reaction:

2 H2O(l) →  2H2(g) + O2(g)

 What mass of H2O is required to form 1.4 L of O2 at a temperature of 315 K and a pressure of 0.957 atm? 

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Consider the chemical reaction:

C(s) + H2O(g) → CO(g) + H2(g)

How many liters of hydrogen gas are formed from the complete reaction of 15.7 g C? Assume that the hydrogen gas is collected at a pressure of 1.0 atm and a temperature of 355 K. 

 

 

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A heliox deep-sea diving mixture contains 2.0 g of oxygen to every 98.0 g of helium. What is the partial pressure of oxygen when this mixture is delivered at a total pressure of 8.5 atm? 

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The zinc within a copper-plated penny will dissolve in hydrochloric acid if the copper coating is filed down in several spots (so that the hydrochloric acid can get to the zinc). The reaction between the acid and the zinc is 2 H+(aq) + Zn(s) → H2(g)+Zn2+(aq). When the zinc in a certain penny dissolves, the total volume of gas collected over water at 25 °C was 0.951 L at a total pressure of 748 mmHg. What mass of hydrogen gas was collected? 


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The air in a bicycle tire is bubbled through water and collected at 25 °C. If the total volume of gas collected is 5.45 L at a temperature of 25°C and a pressure of 745 torr, how many moles of gas were in the bicycle tire?

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The hydrogen gas formed in a chemical reaction is collected over water at 30.0 °C at a total pressure of 732 mmHg. What is the partial pressure of the hydrogen gas collected in this way? If the total volume of gas collected is 722 mL, what mass of hydrogen gas is collected? 

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What is the mole fraction of oxygen gas in air (see Table 5.3)? What volume of air contains 10.0 g of oxygen gas at 273 K and 1.00 atm? 

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A gas mixture contains 1.25 g N2 and 0.85 g O2 in a 1.55-L container at 18 °C. Calculate the mole fraction and partial pressure of each component in the gas mixture. 

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A 1.20-g sample of dry ice is added to a 755-mL flask containing nitrogen gas at a temperature of 25.0 °C and a pressure of 725 mmHg. The dry ice sublimes (converts from solid to gas) and the mixture returns to 25.0 °C. What is the total pressure in the flask? 

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