Problem: An ideal gas at a pressure of 1.60 atm is contained in a bulb of unknown volume. A stopcock is used to connect this bulb with a previously evacuated bulb that has a volume of 0.810 L as shown here. When the stopcock is opened the gas expands into the empty bulb.If the temperature is held constant during this process and the final pressure is 695 torr , what is the volume of the bulb that was originally filled with gas?

FREE Expert Solution

We have to calculate the initial volume of a gas when a gas expands from a pressure of 1.60 atm to a pressure of 695 torr at constant temperature.


We will solve this problem using the Boyle’s law.

Boyle’s law states that the volume of a gas varies inversely with the pressure applied on it.

V  1P


We can remove the proportionality sign to add “=” sign and a constant.

V = constant×1PPV = constant


For two states of a gas:

P1V1 = P2V2

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Problem Details

An ideal gas at a pressure of 1.60 atm is contained in a bulb of unknown volume. A stopcock is used to connect this bulb with a previously evacuated bulb that has a volume of 0.810 L as shown here. When the stopcock is opened the gas expands into the empty bulb.

A flask containing gas is connected by a tube with a stopcock to a smaller empty flask.

If the temperature is held constant during this process and the final pressure is 695 torr , what is the volume of the bulb that was originally filled with gas?