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°C,at what temperature will the pressure of the gas double from its original value?
A)91°C
B)38°C
C)311°C
D)273°C
E)122°C

Question

Quizplus · Accepted Answer

According to Charles's Law, the volume of a gas at constant pressure is directly proportional to its temperature. Since the container is rigid, we can assume that the pressure is constant. Therefore, we can use the ideal gas law:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the universal gas constant, and T is the temperature.

If we double the pressure, we get:

2P = nRT/V

We can see that the only way to double the pressure without changing the number of moles, volume, or gas constant is to double the temperature. Therefore, we need to find the temperature that is double the original temperature of 19°C (which is 292 K):

2T = 2(292 K) = 584 K

Converting this to Celsius, we get:

T = 311°C

Therefore, the answer is choice (C).

A Quantity of an Ideal Gas Is Kept in a Rigid