Question

The following reaction has an equilibrium constant KP equal to 2.4×10-4 at 1073 K..Determine the following at this
temperature.
2H2S(g) ⇌ 2H2(g) + S2(g)
(a) If the reaction favor reactants or products?
(b) KC for the reaction 2H2S(g) ⇌ 2H2(g) + S2(g)?
(c) What is KP for the reaction 3H2(g) + 3/2S2(g) ⇌ 3H2S(g) ?
(d) Determine the reaction quotient for a mixture consisting of 0.212 atm of H2S, 0.677 atm of H2 and 1.14 atm of S2. In which direction will the reaction proceed to reach equilibrium ?
(e) If the equilibrium partial pressures of H2S and S2 are respectively 3.14 atm and 0.107 atm, what is the equilibrium partial pressure of H2 (in atm) ?

The equilibrium reaction: 2NOBr (g) ⇌ 2NO(g) + Br2(g) is endothermic. For each of the following changes indicate if
the concentration of NOBr would decrease, increase, or remain the same {1 point each}
(a) Some Br2 was removed from the reaction mixture ☐ decrease, ☐ increase, ☐ remain the same
(b) The volume of the reaction vessel was increased ☐ decrease, ☐ increase, ☐ remain the same
(c) The temperature of the reaction was increased ☐ decrease, ☐ increase, ☐ remain the same
(d) A catalyst was added ☐ decrease, ☐ increase, ☐ remain the same