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

2b2t

explanation:

2b2t