Question

1. To increase the solubility of a gas at constant temperature from 0.85g/mL at 1.0atm to 5.1g/mL, the pressure would have to be increased to __________. *

Answer 1

Answer : The pressure would have to be increased to 6.0 atm.

Explanation :

According top the Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of the gas.

`S\propto P`

or,

`(S_1)/(S_2)=(P_1)/(P_2)`

where,

`S_1` = initial solubility of gas = 0.85 g/mL

`S_2` = final solubility of gas = 5.1 g/mL

`P_1` = initial pressure of gas = 1.0 atm

`P_2` = final pressure of gas = ?

Now put all the given values in the above formula, we get the final pressure of the gas.

`(0.85g/mL)/(5.1g/mL)=(1.0atm)/(P_2)`

`P_2=6.0atm`

Therefore, the pressure would have to be increased to 6.0 atm.