If more Brions were added to a saturated HgBr2 solution, then the reaction below: HgBr₂(s) Hg2+ (aq) + 2 Br (aq) O A. must shift to the right and consume all the added Br to regain equilibrium. O B. must shift to the right and consume some of the added Br to regain equilibrium. O C. has not been disturbed from its equilibrium position. O D. must shift to the left and consume some of the added Br to regain equilibrium. O E. must shift to the left and consume all the added Br to regain equilibrium.

If more Brions were added to a saturated HgBr2 solution, then the reaction below: HgBr₂(s) Hg2+ (aq) + 2 Br (aq) O A. must shift to the right and consume all the added Br to regain equilibrium. O B. must shift to the right and consume some of the added Br to regain equilibrium. O C. has not been disturbed from its equilibrium position. O D. must shift to the left and consume some of the added Br to regain equilibrium. O E. must shift to the left and consume all the added Br to regain equilibrium.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

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Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.98PAE

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What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
. Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
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A mixture initially consisting of 2 mol CO and 2 mol H2 comes to equilibrium with methanol, CH3OH, as the product: CO(g)+2H2(g)CH3OH(g) At equilibrium, the mixture will contain which of the following? a less than 1 mol CH3OH b 1 mol CH3OH c more than 1 mol CH3OH but less than 2 mol d 2 mol CH3OH e more than 2 mol CH3OH
. True or false? The position of a heterogeneous equilibrium does not depend on the amounts of pure solid or pure liquid reactants or products present because the concentrations of pure solids and liquids cannot change.
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