A sample of gas in a closed container at a temperature of 75◦C and a pressure of 6 atm is heated to 353◦C. What pressure does the gas exert at the higher temperature?

Answer in units of atm.

I got 28.24 and it's wrong

A gas has a pressure of 2.92 atm and occupies a volume of 5.5 L. If the gas is compressed to a volume of 2.61 L, what will its pressure be, assuming constant temperature?
Answer in units of atm.

1. Use (P1/T1) = (P2/T2).

Many students forget to convert temperature from celsius to kelvin.
kelvin = 273.15 + degrees C.

2. Use P1V2 = P2V2

To determine the pressure of a gas at different temperatures or volumes, we can use the ideal gas law equation: PV = nRT. In this equation, P represents pressure, V represents volume, n represents the number of moles of gas, R is the ideal gas constant, and T represents temperature in Kelvin.

For the first question, we need to find the pressure of the gas at the higher temperature. We have the initial temperature T1 = 75°C = 348 K, initial pressure P1 = 6 atm, and final temperature T2 = 353°C = 626 K. We can assume that the number of moles of gas, volume, and the ideal gas constant remain constant. So, to find the final pressure P2, we use the equation:

P1/T1 = P2/T2

Substituting the values we know:

6 atm / 348 K = P2 / 626 K

Solving for P2:

P2 = (6 atm * 626 K) / 348 K ≈ 10.77 atm

Therefore, the gas exerts a pressure of approximately 10.77 atm at the higher temperature.

For the second question, we need to find the pressure of the gas after it is compressed. We have the initial pressure P1 = 2.92 atm, initial volume V1 = 5.5 L, and final volume V2 = 2.61 L. Since the temperature is assumed to remain constant, we can use the equation:

P1 * V1 = P2 * V2

Substituting the known values:

2.92 atm * 5.5 L = P2 * 2.61 L

Solving for P2:

P2 = (2.92 atm * 5.5 L) / 2.61 L ≈ 6.15 atm

Therefore, the pressure of the gas after compression is approximately 6.15 atm.