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

Answer:

$V_2=4.60L$

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:

$V_2=\frac{P_1V_1}{P_2} =\frac{1.50atm*5.00L}{1240mmHg*\frac{1atm}{760mmHg} } \\\\V_2=4.60L$

Regards.