Question

A GAS SAMPLE HAS A TEMPERATURE OF 18 CELSIUS WITH AN UNKNOWN VOLUME. THE SAME GAS HAS A VOLUME OF 436 ML WHEN THE TEMPERATURE IS 91 CELSIUS WITH NO CHANGE IN THE PRESSURE AND AMOUNT OF GAS

Answer 1

Answer : The unknown volume will be, 348.6 mL

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:

$V_1=?\\T_1=18^oC=(18+273)K=291K\\V_2=436mL\\T_2=91^oC=(91+273)K=364K$

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

$\frac{V_1}{291K}=\frac{436mL}{364K}\\\\V_1=348.6mL$

Therefore, the unknown volume will be, 348.6 mL