University of Mississippi

An equilibrium mixture of CO, O2 and CO2 at a certain temperature contains 0.0010 M CO2 and 55) 0.0100 M O2. At this temperature, Kc equals 1.4 × 102 for the reaction: 2 CO(g) + O2(g) ⇌ 2 CO2(g).

For which reaction will Kp = Kc? 54) A) 2 H2O(l) ⇌ 2 H2(g) + O2(g) B) S(s) + O2(g) ⇌ SO2(g) C) K2CO3(s) ⇌ K2O(s) + CO2(g) D) 2 HgO(s) ⇌ Hg(l) + O2(g) E) NiCO3(s) ⇌ NiO(s) + CO2(g)

The reaction below has a Kc value of 61. What is the value of Kp for this reaction at 450 K? 53) N2(g) + 3 H2(g) ⇌ 2 NH3(g)

In which of the following reactions will Kc = Kp? A) CO(g) + 2 H2(g) ⇌ CH3OH(g) B) N2O4(g) ⇌ 2 NO2(g) C) N2(g) + 3 I2(g) ⇌ 2 NI3(g) D) 2 C2H6(g) + 7 O2(g) ⇌ 4 CO2(g) + 6 H2O(g) E) H2(g) + Br2(g) ⇌ 2 HBr(g)

What is ∆n for the following equation in relating Kc to Kp? N2(g) + 3 Br2(g) ⇌ 2 NBr3(g)

) At 900.0 K, the equilibrium constant (Kp) for the following reaction is 0.345. 48) 2 SO2(g) + O2(g) ⇌ 2 SO3(g) At equilibrium, the partial pressure of SO2 is 22.2 atm and that of O2 is 10.1 atm. The partial pressure of SO3 is ________ atm.