At constant volume, if a gas's pressure doubles, what happens to its temperature? (Assume ideal gas behavior.)

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Multiple Choice

At constant volume, if a gas's pressure doubles, what happens to its temperature? (Assume ideal gas behavior.)

Explanation:
At constant volume for an ideal gas, the pressure is directly proportional to temperature when the amount of gas is fixed. This comes from P = nRT/V: with V and n fixed, P ∝ T. So if pressure doubles, temperature must also double to keep the relationship true. Using P1V = nRT1 and P2V = nRT2, dividing the equations gives P2/P1 = T2/T1. If P2 is twice P1, then T2 is twice T1. Therefore, the temperature doubles.

At constant volume for an ideal gas, the pressure is directly proportional to temperature when the amount of gas is fixed. This comes from P = nRT/V: with V and n fixed, P ∝ T. So if pressure doubles, temperature must also double to keep the relationship true. Using P1V = nRT1 and P2V = nRT2, dividing the equations gives P2/P1 = T2/T1. If P2 is twice P1, then T2 is twice T1. Therefore, the temperature doubles.

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