Question

A sample of hydrogen gas at a pressure of 977 mm Hg and a temperature of 32 °C, occupies a volume of 11.3 liters. If the gas is cooled at constant pressure to a temperature of -5 °C, the volume of the gas sample will be L.

Answer 1

Answer : The volume of gas sample will be, 9.93 L

Explanation :

Charles' Law : It states that volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles of gas.

Mathematically,

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

where,

$V_1\text{ and }T_1$ are the initial volume and temperature of the gas.

$V_2\text{ and }T_2$ are the final volume and temperature of the gas.

We are given:

$V_1=11.3L\\T_1=32^oC=(32+273)K=305K\\V_2=?\\T_2=-5^oC=(-5+273)K=268K$

Now put all the given values in above equation, we get:

$\frac{11.3L}{305K}=\frac{V_2}{268K}\\\\V_2=9.93L$

Therefore, the volume of gas sample will be, 9.93 L