What is the pressure in pascals if a force of 4.88 kN is pressed against an area of 235 cm²?

What is the pressure in pascals if a force of 3.44 × 10⁴ MN is pressed against an area of 1.09 km²?

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 × 10²³ 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 N₂ has a volume of 34.65 mL at −196°C. At that temperature, 1 mol of N₂ gas has a volume of 6.318 L if the pressure is 1.000 atm. What pressure is needed to compress the N₂ 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

1. initial volume before ascent?
2. 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

1. initial volume before ascent?
2. 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 N₂ and O₂, 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 N₂ and O₂, 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 CO₂ under these conditions? (The Venusian atmosphere is composed largely of CO₂.)

On the surface of Mars, the atmospheric pressure is 4.50 torr, and the temperature is −87°C. What is the density of CO₂ under these conditions? (The Martian atmosphere, similar to its Venusian counterpart, is composed largely of CO₂.)

HNO₃ reacts with iron metal according to

Fe(s) + 2HNO₃(aq) → Fe(NO₃)₂(aq) + H₂(g)

In a reaction vessel, 23.8 g of Fe are reacted but only 446 mL of H₂ are collected over water at 25°C and a pressure of 733 torr. What is the percent yield of the reaction?

NaHCO₃ is decomposed by heat according to

2NaHCO₃(s) → Na₂CO₃(s) + H₂O(ℓ) + CO₂(g)

If you start with 100.0 g of NaHCO₃ and collect 10.06 L of CO₂ over water at 20°C and 0.977 atm, what is the percent yield of the decomposition reaction?