6.E: Gases (Exercises)
 Page ID
 65022
Additional Exercises
 What is the pressure in pascals if a force of 4.88 kN is pressed against an area of 235 cm^{2}?
 What is the pressure in pascals if a force of 3.44 × 10^{4} MN is pressed against an area of 1.09 km^{2}?
 What is the final temperature of a gas whose initial conditions are 667 mL, 822 torr, and 67°C and whose final volume and pressure are 1.334 L and 2.98 atm, respectively? Assume the amount remains constant.
 What is the final pressure of a gas whose initial conditions are 1.407 L, 2.06 atm, and −67°C and whose final volume and temperature are 608 mL and 449 K, respectively? Assume the amount remains constant.
 Propose a combined gas law that relates volume, pressure, and amount at constant temperature.
 Propose a combined gas law that relates amount, pressure, and temperature at constant volume.
 A sample of 6.022 × 10^{23} particles of gas has a volume of 22.4 L at 0°C and a pressure of 1.000 atm. Although it may seem silly to contemplate, what volume would 1 particle of gas occupy?
 One mole of liquid N_{2} has a volume of 34.65 mL at −196°C. At that temperature, 1 mol of N_{2} gas has a volume of 6.318 L if the pressure is 1.000 atm. What pressure is needed to compress the N_{2} gas to 34.65 mL?
 Use two values of R to determine the ratio between an atmosphere and a torr. Does the number make sense?
 Use two values of R to determine how many joules are in a liter·atmosphere.
 At an altitude of 40 km above the earth’s surface, the atmospheric pressure is 5.00 torr, and the surrounding temperature is −20°C. If a weather balloon is filled with 1.000 mol of He at 760 torr and 22°C, what is its
 initial volume before ascent?
 final volume when it reaches 40 km in altitude? (Assume the pressure of the gas equals the surrounding pressure.)
 If a balloon is filled with 1.000 mol of He at 760 torr and 22°C, what is its
 initial volume before ascent?
 final volume if it descends to the bottom of the Mariana Trench, where the surrounding temperature is 1.4°C and the pressure is 1,060 atm?
 Air, a mixture of mostly N_{2} and O_{2}, can be approximated as having a molar mass of 28.8 g/mol. What is the density of air at 1.00 atm and 22°C? (This is approximately sea level.)
 Air, a mixture of mostly N_{2} and O_{2}, can be approximated as having a molar mass of 28.8 g/mol. What is the density of air at 0.26 atm and −26°C? (This is approximately the atmospheric condition at the summit of Mount Everest.)
 On the surface of Venus, the atmospheric pressure is 91.8 atm, and the temperature is 460°C. What is the density of CO_{2} under these conditions? (The Venusian atmosphere is composed largely of CO_{2}.)
 On the surface of Mars, the atmospheric pressure is 4.50 torr, and the temperature is −87°C. What is the density of CO_{2} under these conditions? (The Martian atmosphere, similar to its Venusian counterpart, is composed largely of CO_{2}.)
 HNO_{3} reacts with iron metal according to
Fe(s) + 2HNO_{3}(aq) → Fe(NO_{3})_{2}(aq) + H_{2}(g)
In a reaction vessel, 23.8 g of Fe are reacted but only 446 mL of H_{2} are collected over water at 25°C and a pressure of 733 torr. What is the percent yield of the reaction?

NaHCO_{3} is decomposed by heat according to
2NaHCO_{3}(s) → Na_{2}CO_{3}(s) + H_{2}O(ℓ) + CO_{2}(g)If you start with 100.0 g of NaHCO_{3} and collect 10.06 L of CO_{2} over water at 20°C and 0.977 atm, what is the percent yield of the decomposition reaction?
Answers
 208,000 Pa
 1,874 K
 \[\frac{P_{1}V_{1}}{n_{1}}=\frac{P_{2}V_{2}}{n_{2}}\]
 3.72 × 10^{−23} L
 1 atm = 760 torr

 24.2 L
 3155 L
 1.19 g/L
 67.2 g/L
 3.99%