# BKC1253: It is intended to mix gas oxygen and gas nitrogen at a temperature of 28 °C. If the mass of gas oxygen is 140.8 g and gas nitrogen is 436.8 g, determine the change in molar Gibbs energy

Question 1

A researcher wishes to determine the molar mass of a metal and a nonvolatile solute. For the metal determination, he dissolves 1.2 g of metal in 100 g of mercury and then the mixture is heated to boiling. For the nonvolatile solute, he dissolves 3.8 g of solute in 300 g water. The properties of mercury and
water are stated in Table 1.

• Determine the molar mass of the metal if the partial pressure of mercury vapor over the boiling mixture is 754 Torr and the vapor pressure of pure mercury is 769 Torr.
• Determine the molar mass of the nonvolatile solute if the mixture freezes at 272.50 K.

Question 2

It is intended to mix gas oxygen and gas nitrogen at a temperature of 28 °C. If the mass of gas oxygen is 140.8 g and gas nitrogen is 436.8 g, determine the change in molar Gibbs energy (in joule unit) when these gases mix. Is the mixing spontaneous?

Question 3

The formation of hydrogen iodide could be obtained from a reversible reaction of hydrogen and iodine as H₂ (g) + I₂ (g) ↔ 2 HI (g). Table 2 shows the thermodynamic values at 298.15 K for the components involved in the reaction. Assume that the vapor behaves as a perfect gas.

• Determine the values of the equilibrium constant at 298.15 K.
• Determine the values of the equilibrium constant at 723.15 K.
A mixture of hydrogen and iodine is placed in a sealed container as Figure 1. Calculate the amounts of all components in the mixture at equilibrium.