Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl'(aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PBCI2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+ : mol/L and %3D Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 103 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-3M is kJ/mol. Show your calculations on the separate sheet of paper.

Consider the reaction: PbCl2(s) → Pb2(aq) + 2 Cl'(aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PBCI2 is dissolved in water at 25°C, what are the concentrations of Pb2 and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+ : mol/L and %3D Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 103 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-3M is kJ/mol. Show your calculations on the separate sheet of paper.

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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For the reaction 4HCI(g) + O2(g)→2H2O(g) + 2C2(g) AH° = -114.4 kJ and AS° = -128.9 J/K The equilibrium constant for this reaction at 267.0 K is Assume that AH° and AS° are independent of temperature.
At what temperature, in °C, is a certain reaction at equilibrium if AH = +83.8 kJ/mol and AS = +170.2 J/mol · K?
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east.cengagenow.com OWLV2 | Online teaching and learning resource from Cengage Le... Use the References to access important values if needed for this questlon. The equilibrium constant, K,, for the following reaction is 0.636 at 600 K. COCI,(g) 2Co(g) + Cl2(g) If AH° for this reaction is 108 kJ, what is the value of K, at 483 K? Kp = Retry Entire Group 1 more group attempt remaining Submit Answer In progress
At - 19.4 °C the pressure equilibrium constant K = 6.3 x 10' for a certain reaction. Here are some facts about the reaction: • The net change in moles of gases is -1. If the reaction is run at constant pressure, the volume increases by 12.%. If the reaction is run at constant pressure, 138. kJ/mol of heat are released. ○ Yes. Using these facts, can you calculate K, at -26. °C? ○ No. If you said yes, then enter your answer at right. Round it to 2 significant digits. at If you said no, can you at least decide whether K -26. °C will be bigger or smaller than K,, at -19.4 °C? 0 Yes, and K,, will be bigger. Yes, and K, will be smaller. ○ No. X
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Calculate A,G° at 25 °C for the formation of 1.00 mol of C2H5 OH(g) from C2H4(g) and H20(g). Use this value to calculate K, for the equilibrium. C2H4 (g) + H2O(g) 2 C,H;OH(g) Use the following data: kJ A;G*, mol C2H4 (g) H2O(g) C2H; OH(g) 68.35 -228.59 -168.49 Kp The v value of A,G' and the v value of Kp indicate that the reaction is product-favored.
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Consider the following equilibrium: 2NH3 (g) = N2 (g)+ 3H, (g) AG = 34. kJ Now suppose a reaction vessel is filled with 7.65 atm of ammonia (NH,) and 0.884 atm of hydrogen (H,) at 600. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? O fall Is it possible to reverse this tendency by adding N,? In other words, if you said the pressure of NH, will tend to rise, can that O yes be changed to a tendency to fall by adding N,? Similarly, if you said the O no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding N,? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N, needed to reverse it. ||atm Round your answer to 2 significant digits.
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