Question

2. A gas container is initially at 40 mm Hg and 77K (liquid nitrogentemperature.) What will the pressure be when the container warmsup to room temperature of 298K?

Answer 1

The final pressure of the gas is 155mmHg

Step-by-step explanation

Given that:

The initial pressure of the gas is 40mmHg

The initial temperature of the gas is 77K

The final temperature of the gas is 298K

To find the final pressure, follow the steps below

In the given data, the volume of the container is fixed. Hence, the process is an Isochoric.

Step1: Write the gas law at constant volume

`(P1)/(T1)=(P2)/(T2)`

Step 2: Substitute the given data into the formula in step 1 to find P2

`\begin{gathered} (40)/(77)=(P2)/(298) \\ \text{ Cross multiply} \\ \text{ 40}*\text{ 298 }=\text{ 77}* P2 \\ 11920\text{ }=\text{ 77}*\text{ P2} \\ \text{ Divide both sides by P2} \\ \text{ P2 }=(11920)/(77) \\ P2\text{ }=154.8mmHg \\ P2\approx155mmHg \end{gathered}`

Hence, the final pressure of the gas is 155mmHg