Question

A sample of hydrogen exerts a pressure of 0.389 ATM and has a volume of 7.0L the pressure increases to 3.35 ATM at constant temperature what will its new volume be

Answer 1

Answer on Question #67784 - Chemistry – General Chemistry

Question:

A sample of hydrogen exerts a pressure of 0.389 ATM and has a volume of 7.0L the pressure increases to 3.35 ATM at constant temperature what will its new volume be?

Solution:

The ideal gas is described by the law

$$PV = nRT,$$

where $P$ is the pressure, $V$ is the volume, $n$ is the amount in moles, $T$ is the temperature, and $R$ is the ideal gas constant. From this law, the volume, $V$ is

$$V = \frac{nRT}{P}.$$

With fixed values of $n$ and $T$ ($R$ is fixed as it is a constant), the volume changes inversely to the pressure:

$$\frac{V_1}{V_2} = \frac{P_2}{P_1} \rightarrow V_2 = \frac{P_1}{P_2} V_1$$

Thus,

$$V_2 = 7 \times 0.389 / 3.35 = 0.813 \text{ (L)}$$

Answer:

The volume of the gas would be 0.813 L.