LAW OF PARTIAL PRESSURE

Question 1

pressures of individual gas components
in the mixture

Answer 1

partial pressures

Question 2

the total pressure of a mixture of gases is just the sum of the pressures that each gas would exert if it were present alone

Answer 2

DALTON’S LAW OF partial pressures

Question 3

a dimensionless quantity that expresses the ratio of
the number of moles of one component to the
number of moles of all components present

Answer 3

MOLE FRACTION

Question 4

A container is filled with N2 , O2 , and Ar gas. The partial pressure of N2 and O2 are 615 torr and 115 torr, respectively. If the total pressure is 800 torr, what is the partial pressure of Ar?

Answer 4

70 torr

Question 5

A storage tank contains 2 mol Ar, 3 mol O2 , and 5 mol N2 at a total pressure of 100 atm. Calculate the partial pressure of each gas.

Answer 5

Ar: 20 atm
O2: 30 atm
N2: 50 atm

Question 6

56 g of N2 and 96 g of O2 are mixed in a 2.0 L container at 300K. Calculate the (a) partial pressure of each gas and (b) the total pressure.

Answer 6

(a) N2 = 24.63 atm
O2 = 36.95 atm
(b) The total pressure = 61.58 atm

Question 7

A 2.0-L vessel holds 3 mol N2 and 2 mol of O2 .
a. What is the mole fraction of N2 and O2 ?
b. If the total pressure inside the container of 57 atm, what is the partial pressure of each gas?

Answer 7

(a)
Mole fraction of N2 = 0.6
Mole fraction of O2 = 0.4

(b)
Partial pressure of N2 = 34.2 atm
Partial pressure of O2 = 22.8 atm

Question 8

A mixture of 4.5% H2 , 76% O2 , and 19.5% N2 has a total pressure of 2.3 atm. What is the partial pressure of each of the gases?

Answer 8

H2 = 0.104 atm
O2 = 1.748 atm
N2 = 0.449 atm