b) 0.0092 M c) 0.011 M 3. Consider the reaction: N2(g) + O2(g) 2NO(g), Ke=0.10 at 2000°C. Starting with initial concentrations of 0.040 mol/L of N2 and 0.040 mol/L of O2, calculate the equilibrium concentration of NO, in mol/L. a) 5.4 x 10-3 M e) 0.10 M f) 0.031 M g) 0.040 M кс Ke z [no]3 Eng][0] FOUR CA BLOSSOM d) 0.080 M h) 0.065 M 2100 поз 00 E нного 0.000 0.100 -X - X +ax e E 0.04-X O.OH-X ах ǝ (0.00545) 20.0114 (ax)d √(o.OH-x)³ ах 0.04-X 4. A sealed chamber contains an equilibrium mixture of NO2(g) and N2O4(g) at 300°C. 0.316 Co.0-xx The partial pressures of NO2 and N2O4 are 1.8 and 24.1 atm, respectively. What is the value of Kp for the dimerization of NO2: 2 NO2(g) N204(g) at 300°C? 25 d) 4.0 e) 7.4 f) 59.3 g) 16.6 h) 23.1 0.01764-0.31/6x +0.3/6x чах +0.3/6x ta316x 0.0126427.316x 2.316x 2.316 (ax)³ (0.44-x) (0.04-x) 250. 102 6316 0.3162

b) 0.0092 M c) 0.011 M 3. Consider the reaction: N2(g) + O2(g) 2NO(g), Ke=0.10 at 2000°C. Starting with initial concentrations of 0.040 mol/L of N2 and 0.040 mol/L of O2, calculate the equilibrium concentration of NO, in mol/L. a) 5.4 x 10-3 M e) 0.10 M f) 0.031 M g) 0.040 M кс Ke z [no]3 Eng][0] FOUR CA BLOSSOM d) 0.080 M h) 0.065 M 2100 поз 00 E нного 0.000 0.100 -X - X +ax e E 0.04-X O.OH-X ах ǝ (0.00545) 20.0114 (ax)d √(o.OH-x)³ ах 0.04-X 4. A sealed chamber contains an equilibrium mixture of NO2(g) and N2O4(g) at 300°C. 0.316 Co.0-xx The partial pressures of NO2 and N2O4 are 1.8 and 24.1 atm, respectively. What is the value of Kp for the dimerization of NO2: 2 NO2(g) N204(g) at 300°C? 25 d) 4.0 e) 7.4 f) 59.3 g) 16.6 h) 23.1 0.01764-0.31/6x +0.3/6x чах +0.3/6x ta316x 0.0126427.316x 2.316x 2.316 (ax)³ (0.44-x) (0.04-x) 250. 102 6316 0.3162

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter15: Principles Of Chemical Reactivity: Equilibria

Section: Chapter Questions

Problem 3PS: Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A...

See similar textbooks

Similar questions

For the reactionH2(g)+I2(g)2HI(g), consider two possibilities: (a) you mix 0.5 mole of each reactant. allow the system to come to equilibrium, and then add another mole of H2 and allow the system to reach equilibrium again. or (b) you mix 1.5 moles of H2 and 0.5 mole of I2 and allow the system to reach equilibrium. Will the final equilibrium mixture be different for the two procedures? Explain.
The following two diagrams represent the composition of an equilibrium mixture for the reaction A2 + B2 2AB at two different temperatures. Based on the diagrams, is the chemical reaction endothermic or exothermic? Explain your answer using Le Chteliers principle. (A atoms are red and B atoms are green in the diagrams.)
Hydrogen and carbon dioxide react at a high temperature to give water and carbon monoxide. H2(g) + CO2(g) H2O(g) + CO(g) (a) Laboratory measurements at 986 C show that there are 0.11 mol each of CO and H2O vapor and 0.087 mol each of H2 and CO2 at equilibrium in a 50.0-L container. Calculate the equilibrium constant for the reaction at 986 C. (b) Suppose 0.010 mol each of H2 and CO2 are placed in a 200.0-L container. When equilibrium is achieved at 986 C, what amounts of CO(g) and H2O(g), in moles, would be present? [Use the value of Kc from part (a).]
A solution is prepared by dissolving 0.050 mol of diiodocyclohexane, C5H10I2, in the solvent CCl4.The total solution volume is 1.00 L When the reaction C6H10I2 C6H10 + I2 has come to equilibrium at 35 C, the concentration of I2 is 0.035 mol/L. (a) What are the concentrations of C6H10I2 and C6H10 at equilibrium? (b) Calculate Kc, the equilibrium constant.
Consider the system 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H20(ℓ) ΔrH° = −1530.4 kJ/mol How will the amount of ammonia at equilibrium be affected by removing O2(g) without changing the total gas volume? adding N2(g) without changing the total gas volume? adding water without changing the total gas volume? expanding the container? increasing the temperature? Which of these changes (i to v) increases the value of K? Which decreases it?
Because calcium carbonate is a sink for CO32- in a lake, the student in Exercise 12.39 decides to go a step further and examine the equilibrium between carbonate ion and CaCOj. The reaction is Ca2+(aq) + COj2_(aq) ** CaCO,(s) The equilibrium constant for this reaction is 2.1 X 10*. If the initial calcium ion concentration is 0.02 AI and the carbonate concentration is 0.03 AI, what are the equilibrium concentrations of the ions? A student is simulating the carbonic acid—hydrogen carbonate equilibrium in a lake: H2COj(aq) H+(aq) + HCO}‘(aq) K = 4.4 X 10"7 She starts with 0.1000 AI carbonic acid. What are the concentrations of all species at equilibrium?
Kc = 5.6 1012 at 500 K for the dissociation of iodine molecules to iodine atoms. I2(g) 2 I(g) A mixture has [I2] = 0.020 mol/Land [I] = 2.0 108 mol/L. Is the reaction at equilibrium (at 500 K)? If not, which way must the reaction proceed to reach equilibrium?
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?
In Section 17.3 of your text, it is mentioned that equilibrium is reached in a closed system. What is meant by the term “closed system,” and why is it necessary for a system to reach equilibrium? Explain why equilibrium is not reached in an open system.
The reaction, 3 H2(g) + N2(g) (g), has the fol lowing equilibrium constants at the temperatures given: atT=25°C,K= 2.8 X 104 at T = 500°C, A = 2.4 X IO"7 At which temperature are reactants favored? At which temperature are products favored? YVhat can you say about the reaction if the equilibrium constant is 1.2 at 127°C?
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?