Question

A sample of gas initially has a volume of 859 ml at 565 k and 2.20 atm. What pressure will the sample have if the volume changes to 268 ml while the temperature is increased to 815 k?

Answer 1

Answer:

10.2 atm

Explanation:

Use ideal gas law:

PV = nRT

Initial number of moles is:

(2.20 atm) (0.859 L) = n (0.0821 atm L / mol / K) (565 K)

n = 0.0407 mol

At the new volume and temperature, the pressure is:

P (0.268 L) = (0.0407 mol) (0.0821 atm L / mol / K) (815 K)

P = 10.2 atm