1 (a) N2(g) O2(g) ZNO (g) AH298 = + 180 kJ mol-! From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalyst

1 (a) N2(g) O2(g) ZNO (g) AH298 = + 180 kJ mol-! From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalyst

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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1 (a) N₂(g) + O₂(g) 2NO (g) AH298 + 180 kJ mol-¹ From the equilibrium shown above, use Le Chatelier's Principle to decide what happens to the equilibrium position by: (a) Increasing the concentration of NO (b) Increasing the pressure (c) Increasing the temperature (d) Increasing the concentration of N2 (e) Adding a catalyst
For the reversible reaction: N 2 (g)+ O 2 (g) = 2 NO (g) AH= 181 kJ (a) What will happen to the concentrations of NO at equilibrium if O, is added? (b) What will happen to the concentrations of NO at equilibrium if NO is removed? (c) What will happen to the concentrations of NO at equilibrium if the volume of the reaction vessel is increased? (d) What will happen to the concentrations of NO at equilibrium if the temperature of the system is decreased? (e) What will happen to the concentrations of N,, 0,, and NO at equilibrium if a catalyst is added?
The following reaction has an equilibrium constant, Kc, of 2.10 x 102 at a particular temperature: N2 (g) + 3 H2 (g) → 2 NH3 (g) +You have a container in which the concentration of N2 is 0.77 M, the the concentration of H2 is 0.84 M, andthe concentration of NH3 is 0.85 M.(a) Calculate the value of the reaction quotient Q.(b) Is the system at equilibrium? If not, predict which way (right or left) the reaction will proceed toreach equilibrium.
Define equilibrium constant Keq
Q3. At 298 K, F3SSF(g) decomposes partially to SF2(g). At equilibrium, the partial pressure of SF2(g) is 1.1X10-4 atm and the partial pressure of F3SSF is 0.0484 atm. (a) Write a balanced equilibrium equation to represent this reaction. (b) Compute the equilibrium constant corresponding to the equation you wrote. (c) Some SF2 (at a partial pressure of 2.3X10-4 atm) is placed in a closed container at 298 K with some F3SSF (at a partial pressure of 0.0484 atm). Enough argon is added to raise the total pressure to 1.000 atm. Calculate the initial reaction quotient for the decomposition of F3SSF to SF2.
A 6.00 mol sample of solid A was placed in a sealed 1.00 L container and allowed to decompose into gaseous B and C. The concentration of B steadily increased until it reached 1.40 M, where it remained constant. A(s)↽−−⇀B(g)+C(g) Then, the container volume was doubled and equilibrium was re‑established. How many moles of A remain? Dont
3. For the following reaction at equilibrium, 2BrNO(g) → 2NO(g) + Br2(g), what will happen if the volume of the container is decreased? (a) The reaction remains unchanged (b) The reaction will shift to the left (c) The reaction will shift to the right
Explain the effect of each of the following stresses on the position of the following equilibrium: 3 NO(g) 2 N¿O(g) + NO2(g) The reaction as written is exothermic. (a) N¿O(g) is added to the equilibrium mixture without change of volume or temperature. (b) The volume of the equilibrium mixture is reduced at constant temperature. (c) The equilibrium mixture is cooled. (d) Gaseous argon (which does not react) is added to the equilibrium mixture while both the total gas pressure and the temperature are kept constant. (e) Gaseous argon is added to the equilibrium mixture without changing the volume.