Question

10.0 grams of a gas occupies 12.5 liters at a pressure of 42.0 mm Hg. What is the volume when the pressure has increased to 75.0 mm Hg? 6.72 L 7.00 L 22.3 L 0.143 L

Answer 1

Answer: 7.00 L

Step-by-step explanation:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature and number of moles.

`P\propto (1)/(V)` (At constant temperature and number of moles)

`P_1V_1=P_2V_2`

where,

`P_1` = initial pressure of gas = 42.0 mm Hg

`P_2` = final pressure of gas = 75.0 mm Hg

`V_1` = initial volume of gas = 12.5 L

`V_2` = final volume of gas = ?

`42.0* 12.5=75.0* V_2`

`V_2=7.00L`

Therefore, the volume when the pressure has increased to 75.0 mm Hg is 7.00 L