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.

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.

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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7. The following exothermic reaction has an established chemical equilibrium. CH4(g) + 2H2S(g)→ CS2(g) + 4H2(g). What would happen to the equilibrium position (shift to the reactants, shift to the products or no shift) if: a. The pressure of the system was reduced. b. The system was cooled down. c. The partial pressure of H2S was reduced. d. More CS2 was added to the system.
Question 16 If the reaction quotient, Q, is less than Kin an equilibrium reaction, then O a. the chemical system has reached equilibrium. O b. the reaction will proceed in the backward direction until equilibrium is established. Oc. the reaction will proceed in the forward direction until equilibrium is established. O d. the temperature must be increased for the reaction to proceed in the forward direction. e. the reaction will proceed in the direction that increases the number of mole of substances.
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The equilibrium constant is equal to 5.00 at 1300 K for the reaction: If initial concentrations are [SO2] = 0.60 M, [O2] = 0.20 M, and [SO3] = 0.50 M, the system is: A. at equilibrium B. Need to know the volume of the container before deciding. C. not at equilibrium and will shift to the right to achieve an equilibrium state D. not at equilibrium and will shift to the left to achieve an equilibrium state E. not at equilibrium and will remain in an unequilibrium state 2 SO2(g) + O2(g) ⇌ 2 SO3(g) Determine how the following changes affect the given equilblirium reaction that is held in a closed container. A(g) + 2 B(s) ⇌ 3 C(g) + 3 D(s) ΔH°rxn = −0.25 kJ/mol Adding some A(g) Adding some D(s) Removing some C(g) Increasing the temperature Halving the volume of the container The following mechanism is proposed for the reaction 2 A2 + B2 → 2 C A2 + B2 → R + C slow A2 + R → C fast What is the rate law…
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…
C2. Subject Chemistry
Consider the following system at equilibrium at 350 K: ? CHĄ(g) + CCl4(g) 2CH,Cl,(g) When some CCI,(g) is removed from the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of CH4 will: | A. Increase. B. Decrease. C. Remain the same.
Consider the reaction 2NO (g) + Cl2 (g) → 2NOCI (g), for which Kc = 6.50 × 104 at 35° C. If the starting concentrations of NO, Cl2 and NOCI are 3.60x103 M, 1.25 M and 5.87 M respectively, in which direction will the reaction proceed to reach equilibrium? a. Depends on the pressure Ob. To the right C. To the left d. The reaction is already at equilibrium
The decomposition of PCl5 occurs by the equilibrium process PCl5(g) = PCl3(g) + Cl2(g) DH, = 92.5 kJ mol–1 If the reaction is initially at equilibrium, explain what happens when the temperature is lowered. Select one: a. The equilibrium shifts left b. The concentration of Cl2(g) will increase c. No change d. The equilibrium shifts right
Consider the following system at equilibrium at 698 K: 2 HI (g)=H2 (g) + I2 (g) When some H2 (g) is added to the equilibrium system at constant temperature: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. It is already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining
Consider the following reaction and its equilibrium constant at some temperature. 2NH3(g) = N₂(g) + 3H₂(g) K₂=35 If the following concentrations are present initially: [NH3] = 0.10 M; [N₂] = 2.00 M; [H₂) = 2.00 M.. Which of the following is correct about the reaction? 1.The reaction is at equilibrium. 2.The reaction is not at equilibrium, it will shift to the left to reach equilibrium. 3.the reaction is not at equilibrium it will shift to the right to reach equilibrium.
Consider the following system at equilibrium at 800 K:2H2(g) + S2(g) = 2H2S(g) + 69.3 kcalIf the TEMPERATURE on the equilibrium system is suddenly increased: The reaction must: A. Run in the forward direction to reestablish equilibrium. B. Run in the reverse direction to reestablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of S2 will: A. Increase. B. Decrease. C. Remain the same.