Question

1. Write down the equilibrium constant expressions, K, and K for each of the following reactions: (a) H2(g)C(g) 2 HCl(g) (b) 2 C(s)+0(g) 2 COg Ag (aq)Cl(aq) (c) AgCl(s) (d) 2 0,(g) 30,(g) 2. A 1.0 L evacuated flask was charged with 0.020 mol of N,O and 0.060 mol of NO, at 25.0 C. After equilibrium was reached the NO2 concentration was found to be 0.0140 M. What is the equilibrium constant K, for the reaction? N,0,(g)2 NO(g) 3. Ammonium sulfide, (NH),S, decompose at 50 C as shown below HS(g) + 2NH,(g) (NH)S(s) If an equilibrium mixture was found to have a H,S concentration of 0.355 M, what is the equilibrium constant, K, for the reaction? 4. What is K, for the above reaction? R 0.08206 L.atm.mol K

Answer 1

9 H2(g) + C2(9) => 2HCl(g): . ke= (hel) () (Che) •Kp = P?Aci - PH2 Pel2 bi 2 C(s) +0(g) => 200C9? Ké = (CO)? (0)?(02) active mass of solid is taken as'?') CO2) kp = pro Por Ş, Agel (s) → Ag(aq) + ce-lae) Xez (Agt) (C) Kez Pagt. Pet ... (AGCI). Pager = (Ag+) (Ct) = Pagt: Per di '20319) = 3019) - Kc = (028 i KP = Poz? (132 P 032.