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* 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 (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* 775mL=P_2* 171mL`

`P_2=2470.03mmHg=2.47* 10^3mmHg`

Therefore, the final pressure of the gas is,
`2.47* 10^3mmHg`