Reviewed CSCA Physics question · Easy

A sealed container holds 2.0 mol of an ideal gas at a pressure of 2.0 × 10^5 Pa and a temperature of 400 K. The gas is heated at constant volume until its temperature reaches 600 K. What is the new pressure of the gas?

3.0 × 10^5 Pa
4.0 × 10^5 Pa
2.5 × 10^5 Pa
1.5 × 10^5 Pa

Show the answer and explanation

Correct answer

A. 3.0 × 10^5 Pa

Principle or equation

For an ideal gas at constant volume, pressure is directly proportional to absolute temperature: P1/T1 = P2/T2.

Why this answer is correct

Using P1/T1 = P2/T2, we have P2 = P1 × (T2/T1) = (2.0 × 10^5 Pa) × (600 K / 400 K) = 3.0 × 10^5 Pa.

Example

If P1 = 1.0 × 10^5 Pa at 300 K, at 450 K the pressure becomes 1.0 × 10^5 × (450/300) = 1.5 × 10^5 Pa.

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