The reaction NO (g) + 03 (g) = NO2 (g) + O2 (g) reaches equilibrium at 310 K. Some of the NO2 gas is then removed from the reaction chamber. Which of the followin hat would result when equilibrium is restored? O a. The concentration of O2 decreases. Ob. The equilibrium constant decreases. Oc. The concentration of NO decreases. Od. The concentration of O3 increases. Oe. The concentration of NO remains the same. Moving to another question will save this response. MacBook Air G 80 F3 :6: F2 F1 2 141 #3 F $4 R 70 % 5 S F5 T 6 & Y 7

The reaction NO (g) + 03 (g) = NO2 (g) + O2 (g) reaches equilibrium at 310 K. Some of the NO2 gas is then removed from the reaction chamber. Which of the followin hat would result when equilibrium is restored? O a. The concentration of O2 decreases. Ob. The equilibrium constant decreases. Oc. The concentration of NO decreases. Od. The concentration of O3 increases. Oe. The concentration of NO remains the same. Moving to another question will save this response. MacBook Air G 80 F3 :6: F2 F1 2 141 #3 F $4 R 70 % 5 S F5 T 6 & Y 7

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter12: Chemical Equilibrium

Section: Chapter Questions

Problem 12.103PAE: 12.103 Methanol, CH3OH, can be produced by the reaction of CO with H2, with the liberation of heat....

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Consider an equilibrium mixture of four chemicals (A, B, C, and D, all gases) reacting in a closed flask according to the equation: A(g)+B(g)C(g)+D(g) a. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer. b. You have the original setup at equilibrium, and you add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is reestablished? Justify your answer.
The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does the equilibrium shift in response to each of the following stresses? (a) The quantity of solid carbon is increased. (b) A small quantity of water is added, and CO2 dissolves in it. (c) The system is cooled. (d) The volume of the container is increased.
Consider the equation G = G + RT ln(Q). What is the value of G for a reaction at equilibrium? What does Q equal at equilibrium? At equilibrium, the previous equation reduces to G = RT ln(K). When G 0, what does it indicate about K? When G 0, what does it indicate about K? When t G = 0, what does it indicate about K? G predicts spontaneity for a reaction, whereas G predicts the equilibrium position. Explain what this statement means. Under what conditions can you use G to determine the spontaneity of a reaction?
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?
Consider the following equilibrium: COBr2(g) CO(g) + Br2(g)Kc = 0.190 at 73 C (a) A 0.50 mol sample of COBr2 is transferred to a 9.50-L flask and heated until equilibrium is attained. Calculate the equilibrium concentrations of each species. (b) The volume of the container is decreased to 4.5 L and the system allowed to return to equilibrium. Calculate the new equilibrium concentrations. (Hint: The calculation will be easier if you view this as a new problem with 0.5 mol of COBr2 transferred to a 4.5-L flask.) (c) What is the effect of decreasing the container volume from 9.50 L to 4.50 L?
. Consider an equilibrium mixture consisting of H2O(g), CO(g). H2(g), and CO2(g) reacting in a closed vessel according to the equation H2O(g)+CO(g)H2(g)+CO2(g)a. You add more H2O to the flask. How does the new equilibrium concentration of each chemical compare to its origin al equilibrium concentration after equilibrium is re-established? Justify your answer. b. You add more H2to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
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Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed flask according to the following equation: A+BC+Da. You add more A to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer. h. You have the original set-up at equilibrium, and add more D to the flask. How does the concentration of each chemical compare to its original concentration after equilibrium is re-established? Justify your answer.
Hydrogen for use in ammonia production is produced by the reaction CH4(g)+H2O(g)750oCNicatalystCO(g)+3H2(g) What will happen to a reaction mixture at equilibrium if a. H2O(g) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert gas is added to a rigid reaction container? d. CO(g) is removed? e. the volume of the container is tripled?
A mixture of N2, H2, and NH3 is at equilibrium [according to the equationN2(g)+3H2(g)2NH3(g)] as depicted below: The volume is suddenly decreased (by increasing the external pressure) and a new equilibrium is established as depicted below: a. If the volume of the final equilibrium mixture is 1.00 L, determine the value of the equilibrium constant, K. for the reaction. Assume temperature is constant. b. Determine the volume of the initial equilibrium mixture assuming a final equilibrium volume of 1.00 L and assuming a constant temperature.
. Consider the reaction 2CO(g)+O2(g)2CO2(g)Suppose the system is already at equilibrium, and then an additional mole of CO2(g) is injected into the system at constant temperature. Does the amount of O2(g) in the system increase or decrease? Does the value of K for the reaction change?