1. X. IfK << 1 (small K value), the equilibrium lies to the right and the products predominate in the equilibrium mixture. mixture. Y. When calculating the value of the equilibrium constant, the concentrations to be used must be equilibrium concentrations. 2. X. HF (aq) → H+ (aq) + F- (aq), the Kc = [HF] / [H+] [F]. Y. C(s) + 2 H2(g) = CH.(g), the Kc = [CH4] / [H.]. 3. X. If reactant predominates, the reaction proceeds in the forward direction until equilibrium is attained. Y. If reactant predominates, the products must react to form the reactants until equilibrium is attained.
1. X. IfK << 1 (small K value), the equilibrium lies to the right and the products predominate in the equilibrium mixture. mixture. Y. When calculating the value of the equilibrium constant, the concentrations to be used must be equilibrium concentrations. 2. X. HF (aq) → H+ (aq) + F- (aq), the Kc = [HF] / [H+] [F]. Y. C(s) + 2 H2(g) = CH.(g), the Kc = [CH4] / [H.]. 3. X. If reactant predominates, the reaction proceeds in the forward direction until equilibrium is attained. Y. If reactant predominates, the products must react to form the reactants until equilibrium is attained.
Introduction to General, Organic and Biochemistry
11th Edition
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Chapter7: Reaction Rates And Chemical Equilibrium
Section: Chapter Questions
Problem 7.81P
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