A 1.18 L sample of gas at 759 mm Hg pressure is expanded until its volume is 2.06 L. What will be the pressure in the expanded gas sample (at constant temperature) ?

434.77 mmHg

Explanation:

Data obtained from the question include:

V1 (initial volume) = 1.18 L

P1 (initial pressure) = 759 mmHg

V2 (final volume) = 2.06 L

P2 (final pressure) = ?

The Boyle's law equation P1V1 = P2V2, will be use to obtain the final pressure of the gas since the temperature is constant. So, applying the Boyle's law equation, the final pressure is obtained as shown below:

P1V1 = P2V2

759 x 1.18 = P2 x 2.06

Divide both side by 2.06

P2 = (759 x 1.18) / 2.06

P2 = 434.77 mmHg

Therefore, the final pressure of the gas is 434.77 mmHg