17.27 (a) Calculate AG° and Kp for the following equilibrium reaction at 25°C. The AG; values are 0 for Cl2(g), -286 kJ/mol for PCI3(g), and -325 kJ/mol for PCI5(g). PCI5 (g) = PCI3 (g) + Cl2 (g) (b) Calculate AG for the reaction if the partial pressures of the initial mixture are PpCI. = 0.0029 atm, PpCI, = 0.27 atm, and %D PCl, = 0.40 atm.

17.27 (a) Calculate AG° and Kp for the following equilibrium reaction at 25°C. The AG; values are 0 for Cl2(g), -286 kJ/mol for PCI3(g), and -325 kJ/mol for PCI5(g). PCI5 (g) = PCI3 (g) + Cl2 (g) (b) Calculate AG for the reaction if the partial pressures of the initial mixture are PpCI. = 0.0029 atm, PpCI, = 0.27 atm, and %D PCl, = 0.40 atm.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 58QAP: Calculate K at 25°C for each of the reactions referred to in Question 32. Assume smallest...

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16) The equilibrium constant for the following reaction at 298 K is Kc=9.1x10−6.2Fe3+(aq) + Hg22+(aq) <--> 2Fe2+(aq) + 2Hg2+(aq)a) What is ΔG° at this temperature?b) If standard-state conditions of the reactants and products are mixed, in which direction does the reaction proceed? c) Calculate ΔG when [Fe 3+]=0.20 M, [Hg22+]=0.010 M, [Fe2+]=0.010 M, and [Hg2+]=0.025 M. In which direction will the reaction proceed to reach equilibrium?
Silver chloride can be formed from metallic silver and hydrogen chloride, based on the reaction: 2 Ag (s) + 2 HCl (g) 2 AgCl (s) + H2 (g) The Gibbs function for the formation, at 25ºC, are the following: For HCl(g) is -95.3 kJ mol-1 and for AgCl(s) is -109.7 kJ mol-1 a) Knowing the reaction constant K = 1.5·103 at 80 ºC, Find the average enthalpy of reaction, considering constant in the range of 0 to 150 ºC. b) Assuming that the gases behave ideally, find the temperature at which, 90% of HCl has reacted at a total pressure of 0.05 atm when it reaches the equilibrium.
Using the axes G vs composition sketch the variation of the Gibbs energy (G) of a reaction mixture with progress of the reaction, if the equilibrium constant for this reaction smaller than 1. Indicate the sign of rG, direction of the spontaneous change along the plot, Gf, products and Gf, reactants (f-formation).
[PtCl4]2- has Kf =1.1 x 1016. Calculate Eored of [PtCl4]2- to Pt at 298 K? Note: Eored of Pt2+ to Pt = +1.20 V.
At 2300 K, the equilibrium constant for the formation of NO (g), is K = 1.7 x 10-3. N2 (g) + O2 (g) NO 2 NO (g) (a) The analysis shows that the concentrations of N2 and O2 are both 0.25 mol L-1, and that ofNO is 0.0042 mol L-1, under certain conditions. Is the system in balance? In caseaffirmative or negative, substantiate your answer.(b) If the system is not in equilibrium, in which direction should the reaction proceed?(c) When the system is in equilibrium, what are the equilibrium concentrations?
The value of ΔG° (kJ/mol) at 25 °C is -20.5. What is the equilibrium constant for this reaction at this temperature expressed with 2 significant digits?
At 380.2 K, the value Kp for the combination reaction of N2 and H2 that produces NH3 gas is 0.00612. What is the equilibrium constant for the decomposition reaction of NH3 at the same temperature that produces N2 and H2?
Another physiological example of an equilibrium system involves the regulation of blood pH. Carbon dioxide in the blood reacts reversibly with water to produce carbonic acid, which dissociates to produce hydronium and bicarbonate ions: CO2 (aq) + H2O (l) ⇔ H2CO3 (aq) ⇔ H3O+ (aq) + HCO3-(aq) Which of the following statement/s is/are TRUE? During strenuous exercise, the amount of carbon dioxide produced by the cells increases as a result of high metabolic activity. The increased concentration of carbon dioxide in the blood causes a shift to the right in this equilibrium to produce more carbonic acid. When this happens, the pH level of the blood increases as hydronium ion concentration increases. One of the body's responses to this imbalance in blood pH is to increase the rate of breathing so more carbon dioxide gas is exhaled from the lungs, thus shifting the equilibrium back to the left and raising the pH back to normal levels. I , II , and III I…
Which of the following statements is true? Select one: At equilibrium, K = 0. If K > 1, the reaction is spontaneous in the reverse direction under standard conditions. For an endothermic reaction, increasing the temperature will increase the value of K. If K = 1×109, equilibrium favours the reactant side. At equilibrium, the concentrations of the reactants are always equal to the concentrations of the products.
Consider the reactions in the table. (a) Write the equilibrium constant in terms of activities for the chemical reaction of fire extinguishers: 2NaHCO3 (s) ↔ Na2CO3 (s) + CO2 (g) + H2O (g) ΔrH = 135.54 KJ (b) At 300 K the equilibrium constant is 3.95x10-6 for the reaction in (a), what is ΔrGo? (c) State in words: what happens to the equilibrium when temperature is increased? Then, verify by finding K for the reaction in (a) at 420 K.
How does the value of ∆G° for a reaction relate to the equilib-rium constant for the reaction? What does a negative ∆G° for a reaction imply about K for the reaction? A positive ∆G°?
Calculate Kp for the following reaction: PCl3 (g) + Cl2 (g) <--> PCl2(g),Kc = 1.67 at 500

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