Use this reaction to answer the question below: Co(H2O)6+ 4 Cl CoCla+ 6H20 (pink) (blue) statement below describes the change that the system will undergo if water is added? 14) More chloride ions will be produced. a. b. More water will be produced. The equilibrium will shift to the right. c. d. The color will become more blue. e. I don't knoww

Use this reaction to answer the question below: Co(H2O)6+ 4 Cl CoCla+ 6H20 (pink) (blue) statement below describes the change that the system will undergo if water is added? 14) More chloride ions will be produced. a. b. More water will be produced. The equilibrium will shift to the right. c. d. The color will become more blue. e. I don't knoww

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 18Q: Consider the following generic reaction: 2A2B(g)2A2(g)+B2(g) Some molecules of A2B are placed in a...

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. Consider the general reaction 2A(g)+B(s)C(g)+3D(g)H=+115kJ/molwhich has already come to equilibrium. Predict whether the equilibrium will shift to the left, will shift to the right, or will not be affected lithe changes indicated below are made to the system. a. Additional B(s) is added to the system. b. C(g) is removed from the system as it forms. c. The volume of the system is decreased by a factor of 2. d. The temperature is increased.
. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?
. Addition of an inert substance (one that does not participate in the reaction) does not change the _________ of an equilibrium.
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?
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Consider the reaction A+BC+D. A friend asks the following: “I know we have been told that if a mixture of A, B, C. and D is in equilibrium and more A is added, more C and D will form. But how can more C and D form if we do not add more B?” What do you tell your friend?
In the figure, orange fish are placed in one aquarium and green fish in an adjoining aquarium. The two tanks are separated by a removable partition that is initially closed. (a) Describe what happens in the first few minutes after the partition is opened. (b) What would you expect to see several hours later? (c) How is this system analogous to dynamic chemical equilibrium?
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?
For the reaction in Question 111, which diagram for Question 111 represents an equilibrium mixture at a temperature below 350 K? a temperature above 350 K? Diagrams for Question 111.
Kp for the following reaction is 0.16 at 25 C: 2 NOBr(g) 2 NO(g) + Br2(g) The enthalpy change for the reaction at standard conditions is + 16.3 kJ/mol-rxn. Predict the effect of the following changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more Br2(g) (b) removing some NOBr(g) (c) decreasing the temperature (d) increasing the container volume
The following is a thought experiment. Imagine that you put a little water in a test tube and add some NaF crystals. Immediately after you add NaF, you observe that the crystals begin dissolving. The quantity of solid NaF decreases, hut before long, it appears that no more NaF is dissolving. The solution is saturated. The equation for the dissolution of NaF in water is NaF(s) —* Na (aq) + F~(aq). As NaF dissolves, what do you think happens to the rate of dissolution? Describe w hat is occurring on the molecular level. Assume that the reverse reaction, Na+(aq) + F“(aq) —* NaF(s), also occurs as the crystal dissolves. In other words, both dissolution and precipitation are taking place. When it appears that there is no more change in the quantin’ of NaF dissolving (the solution is saturated), w hat has happened to the rates of the forward and reverse reactions? Explain your answer.
Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.