標題:
equilibrium constant
發問:
Consider the following equilibrium process at 700°C. 2 H2(g) + S2(g) 2 H2S(g) Analysis shows that there are 2.50 moles of H2, 1.35* 10-5 mole of S2, and 8.70 moles of H2S present in a 12.0 L flask. Calculate the equilibrium constant Kc for the reaction.
最佳解答:
The equilibrium constant is given by: Kc = [H2S]2/[H2]2[S2] From the given: [H2S] = 8.7/12 [H2] = 2.5/12 [S2] = 1.35 × 10-5/12 Therefore, Kc = (8.7/12)2/[(2.5/12)2 × (1.35 × 10-5/12)] = 1.076 × 107 mol-1 dm3
equilibrium constant
發問:
Consider the following equilibrium process at 700°C. 2 H2(g) + S2(g) 2 H2S(g) Analysis shows that there are 2.50 moles of H2, 1.35* 10-5 mole of S2, and 8.70 moles of H2S present in a 12.0 L flask. Calculate the equilibrium constant Kc for the reaction.
最佳解答:
The equilibrium constant is given by: Kc = [H2S]2/[H2]2[S2] From the given: [H2S] = 8.7/12 [H2] = 2.5/12 [S2] = 1.35 × 10-5/12 Therefore, Kc = (8.7/12)2/[(2.5/12)2 × (1.35 × 10-5/12)] = 1.076 × 107 mol-1 dm3
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