A sealed container holds 0.40 mol of an ideal gas at a pressure of 1.5 × 10⁵ Pa and a temperature of 350 K. The gas is heated at constant volume until its temperature reaches 700 K. What is the new pressure of the gas?
Show the answer and explanation
Correct answer
A. 3.0 × 10⁵ 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
Given P₁ = 1.5 × 10⁵ Pa, T₁ = 350 K, and T₂ = 700 K, we solve P₂ = P₁ × (T₂/T₁) = 1.5 × 10⁵ × (700/350) = 3.0 × 10⁵ Pa. The amount of gas and volume remain constant, so the ideal gas law reduces to the direct proportionality.
Example
If a gas at 300 K and 1.0 × 10⁵ Pa is heated to 600 K at constant volume, the new pressure is 2.0 × 10⁵ Pa.
This published item includes a stored explanation and passed the platform’s publication workflow. It is independent preparation material, not a claim of an official or recalled examination question.