5.2.1 The Ideal Gas Law

Question 1

ideal gas law

Answer 1

• The ideal gas law relates the volume, temperature, pressure, and number of moles of an ideal gas in the equation PV = nRT.
• The ideal gas law assumes that the particles of the gas do not occupy much volume relative to the volume of the container and that there are no interactions between gas particles.

Question 2

note

Answer 2

• The ideal gas law relates the volume (V), temperature (T), pressure (P), and number of moles (n) of an ideal gas in the equation PV = nRT.
• R is the universal gas constant.
• R = 0.082058 L · atm/(mol · K).
• An ideal gas is a hypothetical gas that obeys the ideal gas law under all conditions. Many real gases obey the ideal gas law at moderate pressures and temperatures.
• The ideal gas law is based on two assumptions.
• 1) The particles of the gas behave as point particles. This means that the particles of the gas do not occupy much volume relative to the volume of the container.
• 2) There are no interactions between gas particles.
  Real gases obey the ideal gas law under conditions in which these assumptions apply to them.

Question 3

A poisonous gas is being transported from Texas to California. The container is 4000.0 L and 4°C. It can withstand a pressure of 100.0 atm. Which of the following is the maximum safe amount of gas to ship?

Answer 3

1.76 × 10^4 mol

Question 4

The density of a gas at standard temperature is 2.30 g / L. What is the pressure of 1.00 mole of the gas if there are 0.00446 kg of gas present?

Answer 4

11.5 atm

Question 5

There are two 100. ml containers labeled A and B. Container A contains O2 gas and container B contains H2 gas. Both are at STP. Find the number of moles of each gas in each respective cylinder.

Answer 5

O2 4.46 × 10^−3 mol

H2 4.46 × 10^−3 mol

Question 6

According to the ideal gas law, PV = nRT, if the pressure of a gaseous compound in a 2.00 L container is 3.00 atm and the temperature is 20.0°C, how many moles of this compound are present?

Answer 6

0.250 mol

Question 7

There is a canister of carbon dioxide waiting to be shipped out from the warehouse of a popular soft drink manufacturer. The density of CO2 in this container is 0.00183 g / cm3. At a pressure of 1.11 atm, the container will burst. What temperature does the warehouse have to reach before the container will burst if there are 0.0440 kg of CO2 gas in the canister?

Answer 7

52°C

Question 8

What is the pressure exerted by 4.5 mol of a gas in a 15.0 L flask at 285 K?

Answer 8

7.0 atm

Question 9

There is an unlabeled gas cylinder in the chemistry lab. The cylinder contains a gaseous compound. A sample of the compound shows that it contains 27.27% carbon and 72.73% oxygen. The 1.50 L bottle was found at STP and contained 2.94 g of the compound. Identify the number of moles of the compound in the bottle.

Answer 9

0.0669 mol

Question 10

Boyle’s law states that for a gas at constant temperature, volume is inversely proportional to pressure. Charles’ law states that for a gas at constant pressure, volume is directly proportional to temperature. In the ideal gas law, PV = nRT, when V, R, and T are held constant, how is P related to n?

Answer 10

directly proportional

Question 11

Calculate the pressure of 0.800 moles of helium gas, when the gas is in a balloon with a volume of 2.30 L at a temperature of 32°C.

Answer 11

8.71 atm

Question 12

At STP (standard temperature and pressure), there are 0.0357 moles of methane gas (CH4 ) in an 8.0 × 10^2 mL cylinder. What is the pressure exerted by the gas in the cylinder if the temperature is raised from 273 K to 320 K?

Answer 12

1.2 atm