Question

If a gas is cooled from 323.0 K to 273.15 K and volume is keptconstant, what final pressure would result if the original pressure was740.0 mm Hg?

Answer 1

The final pressure of the gas is 626 mmHg

Step-by-step explanation

Given that;

The initial temperature of the gas is 323K

The final temperature of the gas is 273.15K

The original pressure of the container is 740.0mmHg

Follow the process below to find the final pressure of the gas

The provided that shows that the volume remains constant, and this process is called Isochoric.

Step 1: Write the gas law equation at constant volume

`\text{ }(P1)/(T1)=(P2)/(T2)`

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

`\begin{gathered} (740)/(323)=(P2)/(273.15) \\ \text{ Cross multiply} \\ \text{ P2}*\text{ 323 }=\text{ 740}*\text{ 273.15} \\ P2*\text{ 323 }=202131 \\ \text{ Divide both sides by 323} \\ \text{ P2 }=\text{ }(202131)/(323) \\ \text{ P2}=\text{ 625.79 mmHg} \\ P2\approx626\text{ mmHg} \end{gathered}`

Hence, the final pressure of the gas is 626 mmHg