Question

A gas is initially at a pressure of 225 kPa and a temperature of 245 K in a container that is 4.5 L. If the gas is compressed to a volume of 2.1 L and the temperature changes to 275 K, what is the new pressure?

Answer 1

The new pressure of the gas is 475 kPa.

Step-by-step explanation:

To find the new pressure of the gas, we can use the combined gas law equation:

P1V1/T1 = P2V2/T2

Given:

• P1 = 225 kPa (initial pressure)
• V1 = 4.5 L (initial volume)
• T1 = 245 K (initial temperature)
• V2 = 2.1 L (final volume)
• T2 = 275 K (final temperature)

By substituting the values into the equation, we can solve for P2:

P2 = (P1 * V1 * T2) / (V2 * T1)

P2 = (225 kPa * 4.5 L * 275 K) / (2.1 L * 245 K) = 475 kPa

Therefore, the new pressure of the gas is 475 kPa.

Answer 2

Use the ideal gas equation PV=nRT. You can compare before and after using P1V1/n1T1=P2V2/n2T2. Since the number of moles remains constant you can disregard moles from the equation and use pressure, volume and temp. Make sure your pressure is converted to atmospheres, your volume is in liters, and your temperature is in kelvins.