For the reaction Ca(OH)2(aq) + 2HCl(aq) ---> CaCl2(s) + 2H2O(l) Triangle H degree = -30.2 kJ and Triangle S degree = 206 J/K The equilibrium constant for this reaction at 278.0 K is Assume that Triangle H degree and Triangle S degree are independent of temperature.
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Consider the reaction: CaCl2(s) + 2H2O(g) <---> CaCl2•2H2O(s) The equilibrium constant for the reaction as written is: k = [CaCl2 . 2H2O]/[CaCl2][H2O]^2 k = 1 / [H2O]^2 k = 1 / 2[H2O] k = [H2O]^2 k = [CaCl2 . 2H2O]/[H2O]^2
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Consider the following equilibria: Ca(OH)2(s) ⇌⇌ Ca2+(aq) + 2 OH-(aq) K1 = 6.5 x 10-6 H2O(l) ⇌⇌ H+(aq) + OH-(aq) K2 = 1.0 x 10-14 Given these equilibria, what is the equilibrium constant, K, for the following reaction? Ca(OH)2(s) + 2 H+(aq) ⇌⇌ Ca2+(aq) + 2 H2O(l)
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