Question 5 of 13 Submit If Kp is the equilibrium constant for the reaction 2 A (g) + B (g) = 3 C (g). What is the equilibrium constant (in terms of Kp) for the reaction 6 A (g) + 3 B (g) 9 C (g)? A) (K,)/3 A) see problem image B) (Kp)-1/3 B) see problem image (Kp)3 C) see problem image D) see problem image D) (K,)-3 VI 12:42

Question 5 of 13 Submit If Kp is the equilibrium constant for the reaction 2 A (g) + B (g) = 3 C (g). What is the equilibrium constant (in terms of Kp) for the reaction 6 A (g) + 3 B (g) 9 C (g)? A) (K,)/3 A) see problem image B) (Kp)-1/3 B) see problem image (Kp)3 C) see problem image D) see problem image D) (K,)-3 VI 12:42

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

Chapter13: Chemical Equilibrium

Section: Chapter Questions

Problem 123CP: A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless,...

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Nitrogen, hydrogen, and ammonia are in equilibrium in a 1000-L reactor at 550 K. The concentration of N2 is 0.00485 M, H2 is 0.022 M, and NH3 is 0.0016 M. The volume of the container is halved, to 500 L. (a) Calculate the equilibrium constant. (b) Define y as the change in the concentration of nitrogen in the 500-L container. Is y positive or negative? (c) Write the iCe table and express the equilibrium constant in a polynomial in terms of y.
At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?
What is the pressure of BrCl in an equilibrium mixture of Cl2, Br2, and BrCl if the pressure of CI2 in the mixture is 0.115 atm and the pressure of Br2 in the mixture is 0.450 atm? Cl2(g)+Br2(g)2BrCl(g)KP=4.7102
Show that the complete chemical equation, the total ionic equation, and the net ionic equation for the reaction represented by the equation KI(aq)+I2(aq)KI3(aq) give the same expression for the reaction quotient. KI3 is composed of the ions K+ and I3-.
1’he reaction in Exercise 12.33 was repeated. This time, the reaction began when only NO was injected into the reaction container. 110.200 mol L_l NO was injected, what were the equilibrium concentrations of all species? The following reaction establishes equilibrium at 2000 K: N2(g) + O2(g) ^2 NO K = 4.1 X 10~4 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?
At 2000 K, experiments show that the equilibrium constant for the formation of water is 1.6 1010. 2H2(g) + O2(g) 2H2O(g) Calculate the equilibrium constant at the same temperature for H2(g)+12O2(g) H2O(g)
Nitric oxide and bromine at initial partial pressures of 98.4 and 41.3 torr, respectively, were allowed to react at 300. K. At equilibrium the total pressure was 110.5 torr. The reaction is 2NO(g)+Br2(g)2NOBr(g) a. Calculate the value of Kp. b. What would be the partial pressures of all species if NO and Br2, both at an initial partial pressure of 0.30 atm, were allowed to come to equilibrium at this temperature?
Again the experiment in Exercise 12.33 was redesigned. This time, 0.15 mol each of N, and O2 was injected into a 5.0-L container at 2500 K, at which the equilibrium constant is 3.6 X 10-?. What was the composition of the reaction mixture at equilibrium? l'he 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?
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?
7-29 The following reaction was allowed to reach equilibrium at 25°C. Under each component is its equilibrium concentration. Calculate the equilibrium constant, K, for this reaction.
A sample of gaseous nitrosyl bromide (NOBr) was placed in a container tiued with a frictionless, massless piston, where it decomposed at 25C according to the following equation: 2NOBr(g)2NO(g)+Br2(g) The initial density of the system was recorded as 4.495 g/L. After equilibrium was reached, the density was noted to be 4.086 g/L. a. Determine the value of the equilibrium constant K for the reaction. b. If Ar(g) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of K? Explain each answer