Question

1) A gaseous mixture contains 419.0 Torr H2(g),419.0 Torr H2(g), 359.1 Torr N2(g),359.1 Torr N2(g), and 65.7 Torr Ar(g).65.7 Torr Ar(g). Calculate the mole fraction, ?,χ, of each of these gases.

2)

Heliox is a helium‑oxygen mixture that may be used in scuba tanks for divers working at great depths. It is also used medically as a breathing treatment.

A 7.25 L7.25 L tank holds helium gas at a pressure of 1168 psi.1168 psi. A second 7.25 L7.25 L tank holds oxygen at a pressure of 310.6 psi.310.6 psi. The two gases are mixed in a 7.25 L7.25 L tank. If the temperature remains the same throughout the process, what is the pressure of the gas mixture in the tank? Assume ideal gas behavior.

3) Suppose that Daniel has a 3.003.00 L bottle that contains a mixture of O2O2, N2N2, and CO2CO2 under a total pressure of 4.904.90 atm. He knows that the mixture contains 0.310.31 mol N2N2 and that the partial pressure of CO2CO2 is 0.2500.250 atm. If the temperature is 273273 K, what is the partial pressure of O2O2?

4) A 9.65 L9.65 L container holds a mixture of two gases at 27 °C.27 °C. The partial pressures of gas A and gas B, respectively, are 0.155 atm0.155 atm and 0.613 atm.0.613 atm. If 0.200 mol0.200 mol of a third gas is added with no change in volume or temperature, what will the total pressure become?

Answer 1

Solution :-

Q1) Given data

Pressure of each gas

H2 = 419.0 torr

N2 = 359.1 torr

Ar = 65.7 torr

Mole fraction of each gas= ?

Mole fraction = pressure of particular gas / ( total pressure of gases)

Lets calculate the total pressure

Total pressure = pH2 + pN2 + pAr

                          = 419.0 torr + 359.1 torr + 65.7 torr

                          = 843.8 torr

Now lets calculate the mole fraction of each gas

Mole fraction of H2 = pressure of H2 / total pressure

                                     = 419.0 torr / 843.8 torr

                                     = 0.497

Mole fraction of N2 = pressure of N2 /total pressure

                                     = 359.1 torr / 843.8 torr

                                     = 0.426

Mole fraction of Ar =pressure of Ar / total pressure

                                    = 65.7 torr / 843.8 torr

                                    = 0.0778