Question

What is the temperature (in ºC) of a 10.34 g of methane gas, CH4 in a 5.00×10^4 mL vessel at 1010.8 torr?

A sample of gas has an initial pressure of 1.25 atm and an initial volume of 5.0 L. If the volume is changed to 2.0 L, what is the new pressure? Assume temperature and amount remain constant. Express your answer to 3 significant figures.

A sample of gas has an initial pressure of 4.0 atm and an initial volume of 2.0 L. If the pressure is changed to 2.0 atm, what is the new volume? Assume temperature and amount remain constant.

A sample of gas has an initial pressure of 709 mmHg and an initial volume of 395 mL. If the pressure is changed to 1.51 atm, what is the new volume? Assume temperature and amount remain constant. Express your final answer to three significant figures.

Answer 1

The new volume of the gas is 0.243 L.

Step-by-step explanation:

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

P1V1/T1 = P2V2/T2

Given:

• Initial pressure (P1) = 709 mmHg
• Initial volume (V1) = 395 mL
• Final pressure (P2) = 1.51 atm
• Temperature remains constant

First, we need to convert the initial pressure and volume to the same units as the final pressure:

• 1 atm = 760 mmHg
• 1 L = 1000 mL

Converting the initial pressure:

• P1 = 709 mmHg * (1 atm / 760 mmHg) = 0.933 atm

Converting the initial volume:

• V1 = 395 mL * (1 L / 1000 mL) = 0.395 L

Now we can plug the values into the combined gas law equation:

(0.933 atm)(0.395 L) / T1 = (1.51 atm)(V2) / T2

Since the temperature remains constant, T1 = T2, and we can simplify the equation:

(0.933 atm)(0.395 L) = (1.51 atm)(V2)

Solving for V2:

V2 = (0.933 atm)(0.395 L) / (1.51 atm) = 0.243 L

Therefore, the new volume is 0.243 L.