GCEChemistryStates of Matter and Gas Laws2019

The pressure of a gas in a cylinder is 4.0 × 10⁵ Pa at 27°C. If the temperature is raised to 127°C at constant volume, what is the new pressure of the gas?

A$5.33 \times 10^5$ PaCORRECT
B$2.13 \times 10^5$ Pa
C$8.00 \times 10^5$ Pa
D$3.00 \times 10^5$ Pa
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Why the answer is A, and why the others tempt you.
Using Gay-Lussac's Law at constant volume: P₁/T₁ = P₂/T₂. T₁ = 300 K, T₂ = 400 K, P₁ = 4.0 × 10⁵ Pa. P₂ = (4.0 × 10⁵ × 400)/300 = 5.33 × 10⁵ Pa. Option C is a common error from doubling pressure because temperature appears to double in Celsius; option D results from inverting the temperature ratio.
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