9.2 Relating pressure, volume, amount, and temperature: the ideal  (Page 9/19)

A 2.50-L volume of hydrogen measured at –196 °C is warmed to 100 °C. Calculate the volume of the gas at the higher temperature, assuming no change in pressure.

A balloon inflated with three breaths of air has a volume of 1.7 L. At the same temperature and pressure, what is the volume of the balloon if five more same-sized breaths are added to the balloon?

A weather balloon contains 8.80 moles of helium at a pressure of 0.992 atm and a temperature of 25 °C at ground level. What is the volume of the balloon under these conditions?

The volume of an automobile air bag was 66.8 L when inflated at 25 °C with 77.8 g of nitrogen gas. What was the pressure in the bag in kPa?

How many moles of gaseous boron trifluoride, BF ₃ , are contained in a 4.3410-L bulb at 788.0 K if the pressure is 1.220 atm? How many grams of BF ₃ ?

Iodine, I ₂ , is a solid at room temperature but sublimes (converts from a solid into a gas) when warmed. What is the temperature in a 73.3-mL bulb that contains 0.292 g of I ₂ vapor at a pressure of 0.462 atm?

How many grams of gas are present in each of the following cases?

(a) 0.100 L of CO ₂ at 307 torr and 26 °C

(b) 8.75 L of C ₂ H ₄ , at 378.3 kPa and 483 K

(c) 221 mL of Ar at 0.23 torr and –54 °C

A high altitude balloon is filled with 1.41 $\times$ 10 ⁴ L of hydrogen at a temperature of 21 °C and a pressure of 745 torr. What is the volume of the balloon at a height of 20 km, where the temperature is –48 °C and the pressure is 63.1 torr?

A cylinder of medical oxygen has a volume of 35.4 L, and contains O ₂ at a pressure of 151 atm and a temperature of 25 °C. What volume of O ₂ does this correspond to at normal body conditions, that is, 1 atm and 37 °C?

A large scuba tank ( [link] ) with a volume of 18 L is rated for a pressure of 220 bar. The tank is filled at 20 °C and contains enough air to supply 1860 L of air to a diver at a pressure of 2.37 atm (a depth of 45 feet). Was the tank filled to capacity at 20 °C?

A 20.0-L cylinder containing 11.34 kg of butane, C ₄ H ₁₀ , was opened to the atmosphere. Calculate the mass of the gas remaining in the cylinder if it were opened and the gas escaped until the pressure in the cylinder was equal to the atmospheric pressure, 0.983 atm, and a temperature of 27 °C.

While resting, the average 70-kg human male consumes 14 L of pure O ₂ per hour at 25 °C and 100 kPa. How many moles of O ₂ are consumed by a 70 kg man while resting for 1.0 h?

For a given amount of gas showing ideal behavior, draw labeled graphs of:

(a) the variation of P with V

(b) the variation of V with T

(c) the variation of P with T

(d) the variation of $\frac{1}{P}$ with V

A liter of methane gas, CH ₄ , at STP contains more atoms of hydrogen than does a liter of pure hydrogen gas, H ₂ , at STP. Using Avogadro’s law as a starting point, explain why.

The effect of chlorofluorocarbons (such as CCl ₂ F ₂ ) on the depletion of the ozone layer is well known. The use of substitutes, such as CH ₃ CH ₂ F( g ), for the chlorofluorocarbons, has largely corrected the problem. Calculate the volume occupied by 10.0 g of each of these compounds at STP:

(a) CCl ₂ F ₂ ( g )

(b) CH ₃ CH ₂ F( g )

As 1 g of the radioactive element radium decays over 1 year, it produces 1.16 $\times$ 10 ¹⁸ alpha particles (helium nuclei). Each alpha particle becomes an atom of helium gas. What is the pressure in pascal of the helium gas produced if it occupies a volume of 125 mL at a temperature of 25 °C?

A balloon that is 100.21 L at 21 °C and 0.981 atm is released and just barely clears the top of Mount Crumpet in British Columbia. If the final volume of the balloon is 144.53 L at a temperature of 5.24 °C, what is the pressure experienced by the balloon as it clears Mount Crumpet?

If the temperature of a fixed amount of a gas is doubled at constant volume, what happens to the pressure?

If the volume of a fixed amount of a gas is tripled at constant temperature, what happens to the pressure?