The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming no change in moles or temperature?

Name: The pressure of 5.0 L of gas increases from 1.50 atm to 1240 mmHg. What is the final volume of the gas, assuming no change in moles or temperature?
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Question

Quizplus · Accepted Answer

Using Boyle's Law (P1V1 = P2V2), convert 1240 mmHg to atm (1240 mmHg / 760 mmHg/atm = 1.63 atm), then solve for V2: (1.50 atm)(5.0 L) = (1.63 atm)(V2), V2 = 4.6 L.

The Pressure of 5