2. Using the chemical reaction belowN2(g) + O2(g) = 2NO(g); Equilibriumconstant = 0.10 at 2000°CPredict the direction the system will move toattain equilibrium at the given temperature ifwe add1.00 M oxygen (O2) and 1.00 Mnitrogen (N2)а.b.0.50 M nitrogen, 0.500 M oxygen and0.50 NO

The movement of equilibrium reaction is predicted only on the basis of Le Chatelier's Principle. Le…

Answered: 2. Using the chemical reaction below…

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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Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 1.2 x 104 at a certain temperature. If a solid sample of NH.SH decomposes, what will the equilibrium concentration of NH3 be? NH:SH(s) = NH3(g) + H2S(g) 1 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. NH.SH(s) NH:(g) H2S(g) Initial (M) Change (M) Equilibrium (M) RESET 1.2 x 104 +x +2x -2x 1.2 x 104 + x 1.2 x 104 - x 1.2 x 104 + 2x 1.2 x 104- 2x
If Q is the reaction quotient and K is the equilibrium constant, when the constant is at equilibrium what is true? A. Q<K B. Q^2=K C. Q>K D. K^2=QE. Q=K
Consider the equilibrium N₂O4(g) = 2NO₂(g). At 500 °C, the equilibrium mixture contained 3.86 M nitrogen dioxide gas. Calculate the equilibrium concentration of dinitrogen tetroxide if Kc at this temperature is 0.847. Provide your answer to two places after the decimal and without units. Type your answer...
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…
20 <. At a certain temperature, 0.940 mol SO, is placed in a 2.50 L container. 2 SO, (g) =2 SO, (g) + 0,(g) At equilibrium, 0.140 mol O, is present. Calculate Ke. K. = 2.7738 x10-2 Incorrect help about us privacy policy terms of use careers contact us O Bi w
Consider the following reaction: 2 H20(g) + 2 SO2lg)=2 H2S(g) + 3 O2(g) A reaction mixture initially contains 2.8 M H2O and 2.6 M SO2. Determine the equilibrium concentration of H2S if K. for the reaction at this temperature is 1.3 x 106. 0.058 M O 0.028 M O 0.045 M O 0.12 M O 3.1 x 10 M
The equilibrium constant, K, for the following reaction is 1.0 x 10 -5 at 1500 K. N2(g) + O2(g) <---> 2 NO(g) If 0.750 M N2 and 0.750 M O2 are allowed to reach equilibrium at 1500 K, what is the concentration of NO? a. 2.4 x 10-3M b. 6.7 x 10-4M c. 5.5 x 10-3M d. 2.7 x 10-3M e. 1.2 x 10-3M
Consider the following reaction at equilibrium:2SO2(g) + O2 (g) <==> 2SO3(g)Determine if the following changes will increase, decrease or not affect the partial pressure of SO2.a. Decreasing the amount of oxygen in the systemb. Decreasing the volume of the systemc. Decreasing the temperature of the systemd. Decreasing the pressure of the systeme. Adding a catalyst to the reaction system
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
3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: Keq = 4.6 × 10¹ a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) A: shift right b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(g) = 2SO₂(g) + O₂(8) Keq = 0.230 A: shift left A: shift right
For the reaction 2SO2(g) + O2g) 2SO3(2) If K. = 4.3 x 10° and the following concentrations are present: [SO2] = 0.010 M, [SO3] = 10 M, [O2] = 0.01 M. Which of the following statements is correct? A. The system is at equilibrium B. The system is not at equilibrium and is shifting from left to right C. The system is not at equilibrium and is shifting from right to left D. There is not enough information E. The system is at equilibrium and is shifting from left to right 3.
18. Which equilibrium shows a decrease in [products] when the volume decreases? 1. 2H,(g)+O,(g) 2HI(g) d. III and IV 1I a. b. I and II IV e. C.

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2. Using the chemical reaction below N2(g) + O2(g) = 2NO(g); Equilibrium constant = 0.10 at 2000°C Predict the direction the system will move to attain equilibrium at the given temperature if we add 1.00 M oxygen (O2) and 1.00 M nitrogen (N2) а. b. 0.50 M nitrogen, 0.500 M oxygen and 0.50 NO a.