13.2 Exercise 12

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) $2 \text{NH}_{3} \left(g\right) \rightleftharpoons \text{N}_{2} \left(g\right) + 3 \text{H}_{2} \left(g\right) K_{c} = 17 ;$ [NH₃] = 0.20 M, [N₂] = 1.00 M, [H₂] = 1.00 M

(b) $2 \text{NH}_{3} \left(g\right) \rightleftharpoons \text{N}_{2} \left(g\right) + 3 \text{H}_{2} \left(g\right) K_{P} = 6.8 \times 10^{4} ;$ NH₃ = 3.0 atm, N₂ = 2.0 atm, H₂ = 1.0 atm

(c) $2 \text{SO}_{3} \left(g\right) \rightleftharpoons 2 \text{SO}_{2} \left(g\right) + \text{O}_{2} \left(g\right) K_{c} = 0.230 ;$ [SO₃] = 0.00 M, [SO₂] = 1.00 M, [O₂] = 1.00 M

(d) $2 \text{SO}_{3} \left(g\right) \rightleftharpoons 2 \text{SO}_{2} \left(g\right) + \text{O}_{2} \left(g\right) K_{P} = 16.5 ;$ SO₃ = 1.00 atm, SO₂ = 1.00 atm, O₂ = 1.00 atm

(e) $2 \text{NO} \left(g\right) + \text{Cl}_{2} \left(g\right) \rightleftharpoons 2 \text{NOCl} \left(g\right) K_{c} = 4.6 \times 10^{4} ;$ [NO] = 1.00 M, [Cl₂] = 1.00 M, [NOCl] = 0 M

(f) $\text{N}_{2} \left(g\right) + \text{O}_{2} \left(g\right) \rightleftharpoons 2 \text{NO} \left(g\right) K_{P} = 0.050 ;$ NO = 10.0 atm, N₂ = O₂ = 5 atm