Question

Ammonia gas occupies a volume of 67.9 L at a pressure of 632.4 atm. If the pressure were lowered to 356.8 atm, what would the new volume be?

Answer 1

Approximately `120.4` liters.

Explanation:

If the temperature and number of moles is constant, we may use Boyle's law here, which states that

`Pprop1/V`

or

`P_1V_1=P_2V_2`

And so, plugging in the given values, we get,

`632.4 \ "atm"*67.9 \ "L"=356.8 \ "atm"*V_2`

`V_2=(632.4color(red)cancelcolor(black)"atm"*67.9 \ "L")/(356.8color(red)cancelcolor(black)"atm")`

`~~120.4 \ "L"`