Chapter 16, Problem 39
Consider the reaction: N (g) + 3H (g) ⇌ 2NH (g) Complete the table. Assume that all concentrations are equilib- rium concentrations in M. T (K) [n2] [H2] [nH3] Kc 500 0.115 0.105 0.439 575 0.110 ________ 0.128 775 0.120 0.140 ________ ________ 9.6 0.0584
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Calculate Kc for each reaction. b. N2(g) + O2(g) ⇌ 2 NO(g) Kp = 4.10×10^–31 (at 298 K)
Calculate Kp for each reaction. a. I2(g) + Cl2(g) ⇌ 2 ICl(g) Kc = 81.9 (at 298 K)
Calculate Kp for each reaction. b. CH4(g) + H2O(g) ⇌ CO(g) + 3 H2(g) Kc = 1.3×10^22 (at 298 K)
Consider the following reaction: H2(g) + I2(g) ⇌ 2 HI(g) Complete the table. Assume that all concentrations are equilib- rium concentrations in M. T (°C) [H2] [i2] [Hi] Kc 25 0.0355 0.0388 340 ________ 0.0455 445 0.0485 0.0468 0.922 ________ 0.387 9.6 ________ 50.2
Consider the reaction:
2 NO( g) + Br2( g)Δ2 NOBr( g) Kp = 28.4 at 298 K
In a reaction mixture at equilibrium, the partial pressure of NO is 125 torr and that of Br2 is 148 torr. What is the partial pressure of NOBr in this mixture?
Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kp = 2.91*10^3 at 298 K In a reaction at equilibrium, the partial pressure of SO2 is 117 torr and that of Cl2 is 205 torr. What is the partial pressure of SO2Cl2 in this mixture?