D Question 7 If a chemical reaction has an equilibrium constant, K, of 5.00 x 109, what can you say about it that is correct? The reverse reaction rate is very high The reaction favors the products The reaction favors the reactants The forward reaction rate is very high The reaction is likely an aqueous one Question 8 Consider the Haber Process: 3H₂(g) + N₂ (g) = 2NH3(g) If you had a system of hydrogen, nitrogen, and ammonia gas at equilibrium and added more hydrogen gas, what would happen? The reaction would shift in the reverse direction, decreasing the amount of ammonia and making more nitrogen gas Adding more hydrogen gas would have no impact on the system, immediate or long term O The reaction would shift in the forward direction, increasing the concentration of ammonia and nitrogen gas O The reaction would shift in the reverse direction, decreasing the amount of ammonia and nitrogen gas The reaction would shift in the forward direction, increasing the concentration of ammonia and decreasing the concentration of nitrogen gas

D Question 7 If a chemical reaction has an equilibrium constant, K, of 5.00 x 109, what can you say about it that is correct? The reverse reaction rate is very high The reaction favors the products The reaction favors the reactants The forward reaction rate is very high The reaction is likely an aqueous one Question 8 Consider the Haber Process: 3H₂(g) + N₂ (g) = 2NH3(g) If you had a system of hydrogen, nitrogen, and ammonia gas at equilibrium and added more hydrogen gas, what would happen? The reaction would shift in the reverse direction, decreasing the amount of ammonia and making more nitrogen gas Adding more hydrogen gas would have no impact on the system, immediate or long term O The reaction would shift in the forward direction, increasing the concentration of ammonia and nitrogen gas O The reaction would shift in the reverse direction, decreasing the amount of ammonia and nitrogen gas The reaction would shift in the forward direction, increasing the concentration of ammonia and decreasing the concentration of nitrogen gas

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 9RQ: What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at...

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The experiment in Exercise 12.33 was redesigned so that the reaction started with 0.15 mol each of N2 and O2 being injected into a 1.0-L container at 2500 K. The equilibrium constant at 2500 K is 3.6 X 10“’. What was the composition of the reaction mixture after equilibrium was attained? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) *2 2 NO K = 4.1 X IO-4 If the reaction began with 0.100 mol L-1 of N2 and 0.100 mol L-’ ofO2, what were the equilibrium concentrations of all species?
The diagram represents an equilibrium mixture for the reaction N2(g) + O2(g) ⇌ 2 NO(g) Estimate the equilibrium constant.
At 2300 K the equilibrium constant for the formation of NO(g) is 1.7 103. N2(g) + O2(g) 2 NO(g) (a) Analysis shows that the concentrations of N2 and O2 are both 0.25 M, and that of NO is 0.0042 M under certain conditions. Is the system at equilibrium? (b) If the system is not at equilibrium, in which direction does the reaction proceed? (c) When the system is at equilibrium, what are the equilibrium concentrations?
12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat. All species in the reaction are gaseous. What effect will each of the following have on the equilibrium concentration of CO? (a) Pressure is increased, (b) volume of the reaction container is decreased, (c) heat is added, (d) the concentration of CO is increased, (e) some methanol is removed from the container, and (f) H2 is added.
At room temperature, the equilibrium constant Kc for the reaction 2 NO(g) ⇌ N2(g) + O2(g) is 1.4 × 1030. Is this reaction product-favored or reactant-favored? Explain your answer. In the atmosphere at room temperature the concentration of N2 is 0.33 mol/L, and the concentration of O2 is about 25% of that value. Calculate the equilibrium concentration of NO in the atmosphere produced by the reaction of N2 and O2. How does this affect your answer to Question 11?
What is Le Chteliers principle? Consider the reaction 2NOCI(g)2NO(g)+Cl2(g) If this reaction is at equilibrium. what happens when the following changes occur? a. NOCI(g) is added. b. NO(g) is added. c. NOCI(g) is removed. d. Cl2(g) is removed. e. The container volume is decreased. For each of these changes, what happens to the value of K for the reaction as equilibrium is reached again? Give an example of a reaction for which the addition or removal of one of the reactants or products has no effect on the equilibrium position. In general, how will the equilibrium position of a gas-phase reaction be affected if the volume of the reaction vessel changes? Are there reactions that will not have their equilibria shifted by a change in volume? Explain. Why does changing the pressure in a rigid container by adding an inert gas not shift the equilibrium position for a gas-phase reaction?
How does equilibrium represent the balancing of opposing processes? Give an example of an “equilibrium” encountered in everyday life, showing how the processes involved oppose each other.
. For the reaction 3O2(g)2O3(g)The equilibrium constant, K, has the value 1.121054at a particular temperature. a. What does the very small equilibrium constant indicate about the extent to which oxygen gas, O2(g), is converted to ozone gas, O3(g), at this temperature? b. If the equilibrium mixture is analyzed and [O2(g)]is found to be 3.04102M, what is the concentration of O3(g) in the mixture’?
Consider the decomposition of ammonium hydrogen sulfide: NH4HS(s) ⇌ NH3(g) + H2S(g) In a sealed flask at 25 °C are 10.0 g NH4HS, ammonia with a partial pressure of 0.692 atm, and H2S with a partial pressure of 0.0532 atm. When equilibrium is established, it is found that the partial pressure of ammonia has increased by 12.4%. Calculate KP for the decomposition of NH4HS at 25 °C.