A quantity of an ideal gas is kept in a rigid container of constant volume. If the gas is originally at a temperature of $19 ^ { \circ } \mathrm { C }$ at what temperature will the pressure of the gas double from its original value?
A) $273 ^ { \circ } \mathrm { C }$
B) $91 ^ { \circ } \mathrm { C }$
C) $311 ^ { \circ } \mathrm { C }$
D) $122 ^ { \circ } \mathrm { C }$
E) $38 ^ { \circ } \mathrm { C }$

Question

Quizplus · Accepted Answer

For an ideal gas in a rigid container, the pressure is directly proportional to the temperature in Kelvin. To double the pressure, the temperature in Kelvin must also double. The original temperature is $19 ^ { \circ } \mathrm { C }$, which is $19 + 273 = 292 K$. Doubling this gives $584 K$, which is $584 - 273 = 311 ^ { \circ } \mathrm { C }$.

A Quantity of an Ideal Gas Is Kept in a Rigid