Question

Calculate the pressure, in atmospheres, required to compress a sample of helium gas from 27.3 L (at 1.00 atm) to 3.36 L at constant temperature. Enter your answer in the box provided. atm

Answer 1

8.125 atm

Step-by-step explanation:

Hello,

Boyle's law states that at constant temperature:

`P_1V_1=P_2V_2`

In this case:

`P_1=1 atm, V_1=27.3L, V_2=3.36L`

Solving for
`P_2`:

`P_2=(P_1V_1)/(V_2)=(1atm*27.3L)/(3.36L)\\P_2=8.125atm`

Best regards!