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D) The reaction proceeds nearly all the way to completion. 3. Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant is 0. 100 0.080 A) Ke < 1. B) Kc = 0. C) Kc = 1. D) Kc > 1. I 0.000 0.040 0.020 0.000 0.00 1.00 2.00 300 4.00 5.00 Time (min)

D) The reaction proceeds nearly all the way to completion. 3. Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant is 0. 100 0.080 A) Ke < 1. B) Kc = 0. C) Kc = 1. D) Kc > 1. I 0.000 0.040 0.020 0.000 0.00 1.00 2.00 300 4.00 5.00 Time (min)

Chemistry
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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can you explain for question 3 why Kc < 1 based off the graph??
notes ... d6d35969-... 1. The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) 2 HBr(g) 2 HBr(g) = H2(g) + Br2(g) Ke = 3.8 x 10' Kc = ? A) 1.9 × 10* C) 2.6 x 10* E) 1.6 × 103 2. B) 5.3 x 10° D) 6.4 x 10* Which statement is true for a reaction with K, equal to 2.43 x 1012? A) Increasing the temperature will not change the value of K. B) There are appreciable concentrations of both reactants and products. C) The reaction proceeds hardly at all towards completion. D) The reaction proceeds nearly all the way to completion. 3. Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant is 0. 100 A) Ke < 1. B) Kc = 0. C) Kc = 1. D) Kc > 1. 0.080 I 0 060 B. 0.040 A 0.020 0.000 0.00 1.00 2.00 3.00 4.00 5.00 Time (min) 4. In which of the following reactions will Kc = Kp? B) SO3(g) + N0(g) = SO2(g) + NO2(g) D) 2 SO2g) + O2g) = 2 SO3(g) A) 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) C) 2 N2(g) + O2(g) = 2 N20(g) E) None of the above reactions have Kc = Kp. The decomposition of ammonia to nitrogen and hydrogen on a tungsten filament at 800°C is independent of the concentration of ammonia at high pressures of ammonia. What is the order of the reaction with respect to 5.
Transcribed Image Text:notes ... d6d35969-... 1. The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) 2 HBr(g) 2 HBr(g) = H2(g) + Br2(g) Ke = 3.8 x 10' Kc = ? A) 1.9 × 10* C) 2.6 x 10* E) 1.6 × 103 2. B) 5.3 x 10° D) 6.4 x 10* Which statement is true for a reaction with K, equal to 2.43 x 1012? A) Increasing the temperature will not change the value of K. B) There are appreciable concentrations of both reactants and products. C) The reaction proceeds hardly at all towards completion. D) The reaction proceeds nearly all the way to completion. 3. Shown below is a concentration vs. time plot for the reaction A 2B. For this reaction the value of the equilibrium constant is 0. 100 A) Ke < 1. B) Kc = 0. C) Kc = 1. D) Kc > 1. 0.080 I 0 060 B. 0.040 A 0.020 0.000 0.00 1.00 2.00 3.00 4.00 5.00 Time (min) 4. In which of the following reactions will Kc = Kp? B) SO3(g) + N0(g) = SO2(g) + NO2(g) D) 2 SO2g) + O2g) = 2 SO3(g) A) 4 NH3(g) + 3 O2(g) = 2 N2(g) + 6 H2O(g) C) 2 N2(g) + O2(g) = 2 N20(g) E) None of the above reactions have Kc = Kp. The decomposition of ammonia to nitrogen and hydrogen on a tungsten filament at 800°C is independent of the concentration of ammonia at high pressures of ammonia. What is the order of the reaction with respect to 5.
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