Question

Which temperature change would cause the pressure of a gas to double if its volume remains the same?

A. Increasing from 200 K to 400 K
B. Decreasing from 400°C to 200°C
C. Increasing from 20°C to 200°C
D. Increasing from 20°C to 40°C

Answer 1

To double the pressure of a gas while keeping its volume constant, the Kelvin temperature must be doubled. The correct answer is increasing the temperature from 200 K to 400 K, as represented by Option A.

Step-by-step explanation:

The student's question pertains to the relationship between the temperature and pressure of a gas when its volume is held constant, which is described by Gay-Lussac's law. According to this law, for a given amount of gas at constant volume, the pressure is directly proportional to the Kelvin temperature. Therefore, to double the pressure while keeping the volume constant, you need to double the temperature in Kelvin. The only option that reflects this change is increasing the temperature from 200 K to 400 K. If we apply this to the ideal gas law (PV = NkT), and if we double the Kelvin temperature (where T is the absolute temperature in Kelvin), the pressure P will also double, assuming the amount of gas (N) and the volume (V) are constant.

Option A, increasing the temperature from 200 K to 400 K, would indeed cause the pressure to double if the volume remains constant.