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.
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.40PAE: Because carbonic acid undergoes a second ionization, the student in Exercise 12.39 is concerned that...
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![Equilibrium Constant and Le Chatelier's Principle Table
Read each statement and the instruction carefully.
Write A if both statements X and Y are correct. Write B if
statement X is correct, and statement Y is incorrect. Write C if statement X is incorrect, and
statement Y is correct. Write D if both statements X and Y are incorrect. Write your answer on
your answer sheet.
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 (ag) H+ (aq) + F- (ag), the Kc = [HF] / [H+] [F-].
Y. C(s) + 2 H₂(g) → CH4(g), the Kc = [CH4] / [H₂].
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.
4. X. If the Kc of a certain reaction is 1.2 x 10 15 product/s predominates.
Y. If the Kc of a certain reaction is 0.25 and the Qc value is 1.5, product/s dominates.
5. X. To attain equilibrium, Qc must be equal to Kc.
Y. If Q< K, the reaction proceeds in the forward direction until equilibrium is attained.
6. X. If the Kc of a certain reaction is 3.2 x 10-11, the reaction proceeds in the forward direction
until equilibrium is attained.
Y. If the Kc of a certain reaction is 1.25 and the Qc value is 0.75, the reaction proceeds in the
forward direction until equilibrium is attained.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb511ede7-d353-4166-a180-4bedee49e706%2F06603cd8-e14c-4e58-b957-fbaf54dffb70%2Fh2mxuzh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Equilibrium Constant and Le Chatelier's Principle Table
Read each statement and the instruction carefully.
Write A if both statements X and Y are correct. Write B if
statement X is correct, and statement Y is incorrect. Write C if statement X is incorrect, and
statement Y is correct. Write D if both statements X and Y are incorrect. Write your answer on
your answer sheet.
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 (ag) H+ (aq) + F- (ag), the Kc = [HF] / [H+] [F-].
Y. C(s) + 2 H₂(g) → CH4(g), the Kc = [CH4] / [H₂].
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.
4. X. If the Kc of a certain reaction is 1.2 x 10 15 product/s predominates.
Y. If the Kc of a certain reaction is 0.25 and the Qc value is 1.5, product/s dominates.
5. X. To attain equilibrium, Qc must be equal to Kc.
Y. If Q< K, the reaction proceeds in the forward direction until equilibrium is attained.
6. X. If the Kc of a certain reaction is 3.2 x 10-11, the reaction proceeds in the forward direction
until equilibrium is attained.
Y. If the Kc of a certain reaction is 1.25 and the Qc value is 0.75, the reaction proceeds in the
forward direction until equilibrium is attained.
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