A bulb is filled with Hą gas at a temperature T. The pressure is 756 mmHg. A portion of the gas is transferred to a flask and at 100 kPa, occupies 40.0 mL at the same temperature T. The pressure in the original bulb drops to 625 mmHg at temp. T. What is the volume of the bulb? (NOTE: 100 kPA = 750.0 mmHg)

The volume of the bulb is 229.0mL

Explanation:

To solve this question we need to use Boyle's law that states that the pressure is inversely proportional to the volume of a gas under constant temperature. in the problem:

P1V1 = P2V2 + P3V1

Where P is pressure and V volume of:

1, initial state of the gas. 2, state of the transferred flask, 3, final state of the gas in the initial bulb

Replacing:

756mmHg*V1 = 750.0mmHg*40mL + 625mmHg*V1

131mmHg*V1 = 30000mmHg*mL

V1 = 229.0mL

The volume of the bulb is 229.0mL