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Reviewed CSCA Physics question · Standard

A sealed container holds 2.0 mol of an ideal gas at a pressure of 1.0 × 10^5 Pa and a temperature of 300 K. The gas is heated at constant volume until its pressure reaches 2.5 × 10^5 Pa. What is the new temperature of the gas? (Assume ideal gas behavior and R = 8.31 J/(mol·K))

  1. 480 K
  2. 600 K
  3. 750 K
  4. 1200 K
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Correct answer

C. 750 K

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 T2 = T1 × (P2/P1) = 300 K × (2.5 × 10^5 / 1.0 × 10^5) = 300 K × 2.5 = 750 K.

Example

If pressure increases from 1.0 × 10^5 Pa to 2.5 × 10^5 Pa at constant volume, the temperature must increase from 300 K to 750 K.

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