The equilibrium constant, Kp, for the following reaction is 0.497 at 500K. PCI 5(9) PC13 (9) + Cl₂(9) If an equilibrium mixture of the three gases in a 16.9 L container at 500K contains PCIs at a pressure of 0.447 atm and PC13 at a pressure of 0.398 atm, the equilibrium partial pressure of Cl₂ is atm. Submit Answer Retry Entire Group 7 more group attempts remaining

The equilibrium constant, Kp, for the following reaction is 0.497 at 500K. PCI 5(9) PC13 (9) + Cl₂(9) If an equilibrium mixture of the three gases in a 16.9 L container at 500K contains PCIs at a pressure of 0.447 atm and PC13 at a pressure of 0.398 atm, the equilibrium partial pressure of Cl₂ is atm. Submit Answer Retry Entire Group 7 more group attempts remaining

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 33P

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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.
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
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 the following statements: Consider the reaction A(g)+B(g)C(g),for which at equilibrium [A] = 2 M, [B] = 1 M, and [C] = 4 M. To a 1-L container of the system at equilibrium, you add 3 moles of B. A possible equilibrium condition is [A] = 1 M, [B] = 3 M, and [C] = 6 M because in both cases K = 2. Indicate everything that is correct in these statements and everything that is incorrect. Correct the incorrect statements, and explain.
Consider the following hypothetical reaction: X2(g)+R(s)X2R(g) R has a molar mass of 73 g/mol. When equilibrium is established, a 2.5-L reaction vessel at 125C contains 15.0 g of R, 4.3 atm of X2, and 0.98 atm of X2R. (a) Calculate K for the reaction at 125C. (b) The mass of R is doubled. What are the partial pressures of X2 and X2R when equilibrium is reestablished? (c) The partial pressure of X2 is decreased to 2.0 atm. What are the partial pressures of X2 and X2R when equilibrium is reestablished?
For the equilibrium 2 SO2(g) + O2(g) 2 SO3(g) Kc = 245 (at 1000 K) the equilibrium concentrations are [SO2] = 0.102, [O2] = 0.0132, and [SO3] = 0.184. The concentration of SO2 is suddenly doubled. Show that the forward reaction takes place to reach a new equilibrium.
A mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 5.0 103 mol/L, [O2] = 1.9 103 mol/L, and [SO3] = 6.9 103 mol/L. Is the reaction at equilibrium? If not, which way will the reaction proceed to reach equilibrium? 2 SO2(g) + O2(g) 2 SO3(g) Kc = 279
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?
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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?