Question

The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mm Hg. What is the final volume of the gas, assuming constant temperature?

Answer 1

According to Boyles law, V1P1=V2P2
V1=5L
V2=?
P1=1.5atm
P2=1.632atm
Therefore,
5L*1.5atm=1.632atm*V2
V2=5L*1.5atm/1.632atm
=4.596L

Answer 2

4.65 L is the final volume of the gas.

Step-by-step explanation:

Initial pressure of the gas,
`P_1` = 1.50 atm

Initial volume of the gas,
`V_1` = 5.0 L

Final pressure of the gas ,
`P_2`= 1240 mmHg = 1.612 atm

Final Volume of the gas =
`V_2`

Applying Boyle's law:

`P_1V_1=P_2V_2` (Constant temperature)

`V_2=(1.50 atm* 5L)/(1.612 atm)=4.65 L`

4.65 L is the final volume of the gas.