Question

A 1.0 L container holds a sample of hydrogen gas at 300 K and 101.5 k Pa. If the pressure increases to 508 k Pa and the volume remains constant, what will the temperature be?

Answer 1

Answer: The temperature will be 1501.47 K.

Step-by-step explanation:

To calculate the temperature of the gas when pressure is increased, we use the equation given by Gay-Lussac's Law.

This law states that pressure is directly proportional to the temperature of the gas at constant volume and number of moles.

Mathematically,

`P\propto T`

or,

`(P_1)/(T_1)=(P_2)/(T_2)`

where,

`P_1\text{ and }T_1` are the initial pressure and initial temperature of the gas.

`P_2\text{ and }T_2` are the final pressure and final temperature of the gas.

We are given:

`P_1=101.5kPa\\T_1=300K\\P_2=508kPa\\T_2=?K`

Putting values in above equation, we get:

`(101.5kPa)/(300K)=(508kPa)/(T_2)\\\\T_2=1501.47K`

Hence, the temperature will be 1501.47 K