What is the Molar Volume of a Gas at STP?

What is the Molar Volume of a Gas at STP?

The Mole and the Volume of Gas

1. It is rather tricky to find the number of moles of a gas by weighing its mass. Chemists determine the number of moles of any gas by measuring its volume. However, this cannot be done for solids and liquids.
2. It is found that under the same temperature and pressure, equal volumes of all gases contain the same number of particles. Therefore, chemists introduced the concept of molar volume.
3. Molar volume of a gas is defined as the volume of one mole of the gas.
4. Thus, the molar volume is also the volume occupied by 6.02 x 10²³ particles of gas.
5. The molar volume of any gas is 22.4 dm³ mol^-1 at STP or 24 dm³ mol^-1 at room conditions.
   Note: STP refers to standard temperature of 0°C and pressure of 1 atmosphere. Room conditions refer to the temperature of 25°C and the pressure of 1 atmosphere.
6. This means that one mole of any gas occupies the same volume at STP, which is 22.4 dm³. Under room conditions, one mole of any gas occupies 24 dm³.
   Figure above Each of these balloons contains 6.02 x 10²³ gas molecules.
7. The following relationship shows how the volume of a gas can be converted to the number of moles and vice versa.
   
8. In calculations, make sure that the volume of gas and the molar volume are of the same unit, that is, both are in cm³ or both are in dm³. Remember, 1 dm³ = 1000 cm³

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The Mole and the Volume of Gas Problems with Solutions

1. What is the volume of 0.4 mole of carbon dioxide gas at STP?
[Molar volume: 22.4 dm³ mol^-1 at STP]
Solution:
Given the number of moles of carbon dioxide, CO₂ = 0.4 mol
Therefore, the volume of CO₂ = number of moles of CO₂ x molar volume at STP
= 0.4 x 22.4 dm³ = 8.96 dm³

2. Find the number of moles of ammonia gas contained in a sample of 60 cm³ of the gas at room conditions. [Molar volume: 24 dm³ mol^-1 at room conditions]
Solution:

The Relationship Between Mole, Number of particles, Mass and Volume

The following shows the relationships between the number of moles, number of particles, mass and volume of gases.

In most calculations, we first convert other quantities such as the number of particles, mass or volume to the number of moles (refer to Table).
Table: Summary of steps in calculations involving the number of moles

The Relationship Between Mole, Number of particles, Mass and Volume Problems with Solutions

1. What is the volume of 12 g of methane at STP?
[Relative atomic mass: H, 1; C, 12. Molar volume: 22.4 dm³ mol^-1 at STP]
Solution:

2. A sample of 120 cm³ of carbon dioxide is collected at room conditions in an experiment. Calculate the mass of the sample of carbon dioxide.
[Relative atomic mass: C, 12; O, 16. Molar volume: 24 dm³ mol^-1 at room conditions]
Solution:
Given the volume of carbon dioxide, CO₂ = 120 cm³ = 120/1000 dm³ = 0.12 dm³

Therefore, the mass of CO₂ = number of moles of CO₂ × molar mass of CO₂ = 0.005 × [12 + 2(16)]
= 0.005 × 44
= 0.22 g

3. How many hydrogen molecules are there in 6 dm³ of hydrogen gas at room conditions? [Molar volume: 24 dm³ mol^-1 at room conditions. Avogadro constant, NA: 6.02 × 10²³ mol^-1]
Solution:

4. Find the volume of nitrogen gas in cm³ at STP that consists of 2.408 × 10²³ nitrogen molecules. [Molar volume: 22.4 dm³ mol^-1 at STP. Avogadro constant, Na: 6.02 × 10²³ mol^-1]
Solution: