The initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (a) 2NH3(g)⇌N2(g)+3H2(g)Kc=17;2NH3(g)⇌N2(g)+3H2(g)Kc=17; [NH3] = 0.20 M, [N2] = 1.00 M, [H2] = 1.00 M (b) 2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104;2NH3(g)⇌N2(g)+3H2(g)KP=6.8×104; NH3 = 3.0 atm, N2 = 2.0 atm, H2 = 1.0 atm (c) 2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230;2SO3(g)⇌2SO2(g)+O2(g)Kc=0.230; [SO3] = 0.00 M, [SO2] = 1.00 M, [O2] = 1.00 M

The first step in HNO3 production is the catalyzed oxidation of NH3. Without a catalyst, a different reaction predominates: 4 NH3(g) +3 O2 (g) ⇌ 2 N2(g) + 6 H2O(g) When 0.0150 mol of NH3(g) and 0.0150 mol of O2(g) are placed in a 1.00−L container at a certain temperature, the N2 concentration at equilibrium is 1.96 ×10−3 M. Calculate Kc.

-2 The equilibrium constant K,, for the following reaction is 7.73×10atmat 350°C. What is the value of K. for the reaction at the same temperature? N2(g) +3H2(g)→ 2NH3(g)

Nitrogen and hydrogen react to form ammonia, like this: N2 (g)+3H,(g) 2NH;(g) Suppose a mixture of N,, H, and NH, has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. alo perturbation change in composition shift in equilibrium Ar to the right The pressure of N, will to the left Some H, is removed. The pressure of NH, will (none) to the right The pressure of N, will ? to the left Some NH, is added. The pressure of H, will v ? O (none) go up. go down. not change.