Question

(1). What is the volume of one mole of hydrogen gas at 273 K and 760 torr?

(2). What is the volume of one mole of oxygen gas under the same conditions?

(3). What does this suggest concerning the ideal gas law?

(4). Show how Boyle's and Charles' laws may be derived from the ideal gas law.

Answer 1

First, note that we will assume ideal gas law

PV = nRT always valid

so

(1). What is the volume of one mole of hydrogen gas at 273 K and 760 torr?

PV = nRT

V = nRT/P

V = (1)(62.4)(273)/(760) = 22.414L

(2). What is the volume of one mole of oxygen gas under the same conditions?

the volume should be the same, since 1 mol of any gas occupies the same space at same conditions

(3). What does this suggest concerning the ideal gas law?

This is applicable for any ideal gas

(4). Show how Boyle's and Charles' laws may be derived from the ideal gas law.

From the ideal gas

for Boyle law:

P1*V1 = C = P2*V2

For Charles law

V2/T1 = C = V2/T2