4. The diagram below shows the changes in concentrations of three substances,X, Y, Z, as they take part in a chemical reaction that reaches equilibrium. Allthree substances are gases.Reaction ProgressTime (minn).a) Write an equation to describe the equilibrium.b) Predict how the graph will change if more of compound Z is added at10 min. Give reasons for your prediction.

We are given the graph of concentration vs time.

4. The diagram below shows the changes in concentrations of three substances, X, Y, Z. as they take part in a chemical reaction that reaches equilibrium. All three substances are gases. Reaction Progress s78 Time (min) a) Write an equation to describe the equilibrium. b) Predict how the graph will change if more of compound Z is added at 10 min. Give reasons for your prediction.

4. The diagram below shows the changes in concentrations of three substances, X, Y, Z. as they take part in a chemical reaction that reaches equilibrium. All three substances are gases. Reaction Progress s78 Time (min) a) Write an equation to describe the equilibrium. b) Predict how the graph will change if more of compound Z is added at 10 min. Give reasons for your prediction.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 51QAP: . For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular...

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Similar questions

The equilibrium between nitrogen monoxide, oxygen, and nitrogen dioxide may be expressed in the equation 2NO(g)+O2(g)2NO(g). Write the equilibrium constant expression for this equation. Then express the same equilibrium in at least two other ways, and write the equilibrium constant expression for each. Are the constants numerically equal? Cite some evidence to support your answer. Nitrogen monoxide and oxygen, both colorless gases, react to form reddish-brown nitrogen dioxide.
Consider the reaction N2O4(g)2NO2(g). Draw a graph illustrating the changes of concentrations of N2O4 and NO2 as equilibrium is approached. Describe how the rates of the forward and reverse reactions change as the mixture approaches dynamic equilibrium. Why is this called a dynamic equilibrium?
. In general terms. what does the equilibrium constant for a reaction represent? What is the algebraic form of the equilibrium constant for a typical reaction? What do square brackets indicate when we write an equilibrium constant?
Consider the following equilibrium constants. Describe how you would expect the equilibrium concentrations of reactants and products to compare with each other larger than, smaller than, etc. for each case. a. K=2.1106 b. K=0.15 c. K=1.2108 d. K=0.00036
The following series of diagrams represent the reaction XY followed over a period of time. The X molecules are red and the Y molecules are green. At the end of the time period depicted, has the reaction system reached equilibrium? Justify your answer with a one-sentence explanation.
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
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.
Calculate the equilibrium concentrations that result when 0.25 M O2 and 1.0 M HCl react and come to equilibrium. 4HCl(g)+O2(g)2Cl2+2H2O(g)Kc=3.11013

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