Question 3 Consider the following reaction, which is initially at equilibrium. What happens when HX is added to the equilibrium mixture? HX(aq) + H*(aq) + X'(aq) O The reaction shifts right because a product was removed. O The reaction doe not shift left or right because the equilibrium position was not affected. O The reaction shifts right because a reactant was added. O The reaction shifts left because a product was added. O The reaction shifts left because a reactant was removed.

Question 3 Consider the following reaction, which is initially at equilibrium. What happens when HX is added to the equilibrium mixture? HX(aq) + H*(aq) + X'(aq) O The reaction shifts right because a product was removed. O The reaction doe not shift left or right because the equilibrium position was not affected. O The reaction shifts right because a reactant was added. O The reaction shifts left because a product was added. O The reaction shifts left because a reactant was removed.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 9RQ: What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at...

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Consider the following generic reaction: 2A2B(g)2A2(g)+B2(g) Some molecules of A2B are placed in a 1.0-L container. As time passes, several snapshots of the reaction mixture are taken as illustrated below. Which illustration is the first to represent an equilibrium mixture? Explain. How many molecules of A2B reacted initially?
A chemist put 1.18 mol of substance A and 2.85 mol of substance B into a 10.0-L flask, which she then closed. A and B react by the following equation: A(g)+2B(g)3C(g)+D(g) She found that the equilibrium mixture at 25C contained 0.376 mol of D. How many moles of B are in the flask at equilibrium at 25C? a 2.47 mol b 3.60 mol c 2.52 mol d 2.10 mol e 2.41 mol
Consider the system SO3(g)SO2(g)+12 O2(g)H=98.9kJ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by 1. adding oxygen gas. 2. compressing the system at constant temperature. 3. adding argon gas. 4. removing SO2(g). 5. decreasing the temperature. (b) Which of the above factors will increase the value of K? Which will decrease it?
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 of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
If the concentrations of products and reactants are equal, is the system at equilibrium?
Consider the following system: 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=153.04kJ (a) How will the amount of ammonia at equilibrium be affected by (1) removing O2(g) ? (2) adding N2(g)? (3) adding water N2(g) ? (4) expanding the container at constant pressure? (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?
Consider the isomerization of butane with an equilibrium constant of K = 2.5. (See Study Question 13.) The system is originally at equilibrium with [butane] = 1.0 M and [isobutane] = 2.5 M. (a) If 0.50 mol/L of isobutane is suddenly added and the system shifts to a new equilibrium position, what is the equilibrium concentration of each gas? (b) If 0.50 mol/L of butane is added to the original equilibrium mixture and the system shifts to a new equilibrium position, what is the equilibrium concentration of each gas?
Pure iron metal can be produced by the reduction of iron(III) oxide with hydrogen gas. (a) Write the expression for the equilibrium constant (Kc) for the reversible reaction Fe2O3(s)+3H2(g)2Fe(s)+3H2O(g)H=98.7kJ (b) What will happen to the concentration of each reactant and product at equilibrium if more Fe is added? (c) What will happen to the concentration of each reactant and product at equilibrium if H2O is removed? (d) What will happen to the concentration of each reactant and product at equilibrium if H2 is added? (e) What will happen to the concentration of each reactant and product at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel? (d) What will happen to the concentration of each reactant and product at equilibrium if the temperature of the system is increased?
Write an equilibrium expression for each of the following gaseous reactions: a.3O22O3 b.COCl2CO+Cl2 c.CS2+4H2CH4+2H2S d.2SO2+O22SO3 e.CO+H2OCO2+H2
Write equilibrium expressions for each of the following equilibria. 2 C(s) + O2(g) «=* 2 CO(g) Zn (aq) + H2S(g) *=* ZnS(s) + 2 H (aq) HCl(g) + H2O(€) 5=i H,O+(aq) + Cl"(aq) (d) H2(g) + | O2(g) s=s H2O(g)