Question

The pressure of a sample of helium in a 1L container is .988 atm. What is the new pressure if the sample is placed in a 2L container?

Answer 1

The new pressure will be 0.494 atm.

Step-by-step explanation:

We can use the ideal gas law to solve this problem:

PV = nRT

where:

• P is the pressure
• V is the volume
• n is the number of moles of gas
• R is the ideal gas constant
• T is the temperature

We know that the initial pressure is 0.988 atm, the initial volume is 1 L, and the temperature is constant.

We also know that the final volume is 2 L.

We can solve for the final pressure as follows:

`P_2 = (P_1V_1)/(V_2)`

substituting value

`P_2 = (0.988\: atm*1 L)/(2 L)`

`P_2 = 0.494 atm`

Therefore, the new pressure will be 0.494 atm.