Question

The pressure of 5.00 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming constant temperature?

Answer 1

(P1)(V1)=(P2)(V2)
(1.50)(5.00)=(1240/760)(V2)
(7.5)/(1240/760)=V2
V2=4.596774194 L

Answer 2

`V_2=4.60L`

Step-by-step explanation:

Hello,

In this case, by means of the Boyle's law which allows us to understand a gas' volume-pressure relationship through an inversely proportional relationship:

`P_1V_1=P_2V_2`

We solve for the final volume
`V_2` as required, including the conversion from mmHg to atm for the final pressure:

`V_2=(P_1V_1)/(P_2) =(1.50atm*5.00L)/(1240mmHg*(1atm)/(760mmHg) ) \\\\V_2=4.60L`

Regards.