Question

A sample of chlorine gas occupies a volume of 775 mL at a pressure of 545 mmHg. Calculate the pressure of the gas (in mmHg) if the volume is reduced at constant temperature to 171 mL. Enter your answer in scientific notation.

Answer 1

Answer : The final pressure of the gas is, $2.47\times 10^3mmHg$

Explanation :

Boyle's Law : It is defined as the pressure of the gas is inversely proportional to the volume of the gas at constant temperature and number of moles.

$P\propto \frac{1}{V}$

or,

$P_1V_1=P_2V_2$

where,

$P_1$ = initial pressure = 545 mmHg

$P_2$ = final pressure = ?

$V_1$ = initial volume = 775 mL

$V_2$ = second volume = 171 mL

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

$545mmHg\times 775mL=P_2\times 171mL$

$P_2=2470.03mmHg=2.47\times 10^3mmHg$

Therefore, the final pressure of the gas is, $2.47\times 10^3mmHg$