Question

A sample of helium gas initially at 37.0°C, 785 torr and 2.00 L was heated to 58.0°C while the volume expanded to 3.24 L. What is the final pressure in atm?

Answer 1

Combined gas law:
`(P_1V_1)/T_1=(P_2V_2)/T_2`

You want to solve for `P_2`:
So: `P_2=(P_1V_1T_2)/(T_1V_2)`

Convert each given temperature to Kelvin:
`37°C+273= 310 K`
`58°C+ 273 = 331K`

Plug in givens:
`P_2=((785 "torr")(2.00 L)(331 K))/((310. K)(3.24 L))`

`P_2 approx 517 " torr"`