7.15a gomThe equilibriumPC15(g) PC13(g) + Cl2(g)has Kp = 0.75 atm. The partial pressure of Cl2 at equilibrium is 0.45 atm. What is thetotal pressure at equilibrium given that PCl5 was pure when introduced into anevacuated container and allowed to decompose to reach equilibrium with PC13 andCl₂?

Approach to solving the question:An equilibrium table should be first tabulated. As the initial…

Answered: 7.15 a gom The equilibrium PC15(g)…

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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The equilibrium constant, Kp , for the following reaction is 0.215 at 673 K.NH4I(s) NH3(g) + HI(g)If an equilibrium mixture of the three compounds in a 7.23 L container at 673 K contains 2.70 mol of NH4I(s) and 0.128 mol of NH3(g), the partial pressure of HI(g) is atm.
A reaction is prepared by adding 2.000 mol each of H2, 12, and HI gases to a 1.0 L container. They are allowed to come to equilibrium, following the reaction: H2 (g) + I2(9) = 2HI(g) At the steady-state, 0.743 mol of HI remained in the container. What is the equilibrium constant Kc for this reaction under these conditions?
The decomposition of HI at low temperature was studied by injecting 2.50 mol of HI into a 10.32-L vessel at 25℃. What is [H2] at equilibrium for the reaction 2HI(g) H2(g) + I2(g); Kc = 1.2610-3 ?
For a particular reaction K = 98000. What can be said about this reaction? A) There are many more products than reactants in the equilibrium mixture. B) There are many more reactants than products in the equilibrium mixture. C) There are roughly equal amounts of reactants and products in the equilibrium mixture. D) The reaction has not yet reached equilibrium because K does not equal 1.
Please don't provide handwritten solution .....
The equilibrium constant, Kp, for the following reaction is 2.20x10 at 723K. 2NH3(g) N3(g)+3H3(g) If an equilibrium mixture of the three gases in a 11.3 L container at 723K contains NH at a pressure of 1.27 atm and N, at a pressure of 0.599 atm, the equilibrium partial pressure of H, is atm.
A pure sample of SO3 is placed in a container and reacts according to the equation 2 SO3(g) ⇄ 2 SO2(g) + O2(g) Kp = 4.00At equilibrium the partial pressure of O2 is 0.10 atm. Calculate the pressure of SO3 remaining at equilibrium.
Consider the following equilibrium reaction: 2NO (g) + Cl2 (g) 2 NOCl (g) K=12 At equilibrium, [NOCl] = 1.60 M and [NO] = 0.80 M. The [Cl2] is
The reaction H2(g) + I2(g) 2HI(g) has Kp = 45.9 at 763 K. A particular equilibrium mixture at 763 K contains HI at a pressure of 3.01 atm and H2 at a pressure of 2.62 atm. Calculate the equilibrium pressure of I2(g) in this mixture.
Gaseous NO is placed in a closed container at 477 oC, where it partially decomposes to NO2 and N2O: 3 NO(g) 1 NO2(g) + 1 N2O(g) At equilibrium it is found that p(NO) = 0.009840 atm, p(NO2) = 0.008270 atm, and p(N2O) = 0.008870 atm. What is the value of KP at this temperature?KP =
Consider the following reaction:2NOBr(g) 2NO(g) + Br2(g) If 0.224 moles of NOBr, 0.330 moles of NO, and 0.384 moles of Br2 are at equilibrium in a 14.0 L container at 518 K, the value of the equilibrium constant, Kp, is .
The equilibrium constant Kp for the reaction,2 SO3(g) <-------> 2 SO2(g) + O2(g)is 7.880 at 759 °C. If a vessel at this temperature initially contains pure SO3 and if the partial pressure of SO3 at equilibrium is 0.109 atm, what is the partial pressure of O2 in the flask at equilibrium? What was the initial pressure of SO3 in the flask?

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