If we represent the equilibrium as: 2 NO2(g)= N½0¼(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. | 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. |3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

If we represent the equilibrium as: 2 NO2(g)= N½0¼(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. | 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. |3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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If we represent the equilibrium as:...Co2+(aq) + 4Cl-(aq) CoCl42-(aq)We can conclude that: fill in the blank 1 1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. fill in the blank 2 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. fill in the blank 3 3. When the temperature is increased the equilibrium concentration of Co2+: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. Consider the following system at equilibrium at 600 K:COCl2 (g) CO (g) + Cl2 (g)If the PRESSURE of the equilibrium system is suddenly decreased at constant temperature: The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to…
If we represent the equilibrium as: 2 NO2(g) = N204(g) We can conclude that: |1. This reaction is: A. Exothermic B. Endothermic C. Neutral D. More information is needed to answer this question. 2. When the temperature is increased the equilibrium constant, K: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question. 3. When the temperature is increased the equilibrium concentration of NO2: A. Increases B. Decreases C. Remains the same D. More information is needed to answer this question.
20. What will happen to the equilibrium when more SO2 (g) is added to the following system? 2502(g) + O2(g) = 250(g) A. It will shift to the right. B. It will shift to the left C. no shift of equilibrium D. cannot be determined 21. For the reaction 2A+B2C the appropriate form for the equilibrium constant expression is: A. [A][B12/ [C] B. [AB]/[C12 C. [C]2/[A][B] D. [ABRIC] 22. Calculate K for the following reaction given the following equilibrium concentrations of H2, CO, and H₂O. PCl3(g) + Cl₂(g) K=? Equilibrium Concentrations (M): PCIs(g) .200 .040 .080 A. 0.16 B.0.016 C.1.6 D.16 23. Which of the following is not omitted when writing the equilibrium constant expression? D. all of the choices A. gas C. solid B. liquid 24. When can we say that the reaction is already at equilibrium? A. When Q is not equal to K. C. When Q is greater than K. D. When Q is lesser than K. B. When Q is equal to K. 25. Where will the equilibrium shift when we increase the pressure of the system? B. towards…
The equilibrium constant of Br2(g) + F2(g) + 2BRF(g) is 54.7. Calculate the equilibrium concentration of BrF if the initial concentrations of Br2 and F2 are 0.25 mol/L? а. 1.25 b. 0.72 О с. 0.38 O d. 0.555 е. 0.205
MAI Van JL.cas-Cudo Lab Assignment #3 E.mheducation.com Saved # 3 6 Be sure to answer all parts. Consider the following equilibrium system involving SO2, Cl2, and SO,Cl, (sulfuryl dichloride): SO2(g) + Cl2(g) = SO,C(g) Predict how the equilibrium position would change if the following changes were to occur. The temperature remains constant in each case. (a) Cl, gas is added to the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. ((More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (b) SO,Cl, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More reactants form.) The equilibrium position will shift to favor the forward reaction. (More products form.) (c) SO, is removed from the system. The equilibrium will not change. The equilibrium position will shift to favor the reverse reaction. (More…
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A k value above 1 means. A. Equilibrium has been reached yet B. Equilibrium favors neither side C. Equilibrium favors reactants D. Equilibrium favors products
If the equilibrium constant, K, is greater than 1 which of the following is true? Select one: a. There are more products than reactants. b. There are more reactants than products. O c. We have all reactants and zero products. O d. The number of reactants equals the number of products.
f the value of Q is greater than K for an equilibrium reaction then a. a catalyst is necessary to achieve equilibrium. b. the reaction will proceed to the right until equilibrium is established. c. the reaction will proceed to the left until equilibrium is extablished. d. the reaction will go left or right depending on the reaction stoichiometry. e. Both (a) and (d) are correct.
Write the equilibrium expression for 2NO(g) + 2H2(g) = N2(g) + 2H20(g). a. Ke = [H20]2 [N2] / [NO]² [H2]² O b. Kc [N2]/ [NO]2 [H2]? %3D O c. Ke [NO]? [H2]? / [H2O]² [N2] %3D