Question

1) At a certain temperature, a 24.0-L contains holds four gases in equilibrium. Their masses are: 3.5 g SO3, 4.6 g SO2, 11.4 g N2, and 0.98 g N2O. What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3 and N2 (balanced with lowest whole-number coefficients)? Kc ==> ?

2) Phosphorus pentachloride decomposes according to the chemical equation: PCl5(g) -><- PCl3(g) + Cl2(g)

Kc = 1.80 @ 250 Celius

A 0.273 mol sample of PCl5(g) is injected into an empty 3.95 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.

PCl5 = ___ M

PCl3 = ___M

3) At a certain temperature, the Kp for the decomposition of H2S is 0.758. H2S(g) -><- H2(g) + S(g)

Initially, only H2S is present at a pressure of 0.187 atm in a closed container. What is the total pressure in the container at equilibrium?

--> ?? atm

Answer 1