(a) Formulate the equilibrium expression for the endo-thermic reactionAgCl-NH3(s) = A£CI(s) + NH3(g)(b) What is the effect on PNH, at equilibrium if addi-tional AgCl(s) is added?(c) What is the effect on PNH, at equilibrium if addi-tional NH3(g) is pumped into or out of the system,provided that neither of the two solid phases shownin the chemical equation is completely used up?(d) What is the effect on PNH; of lowering thetemperature?

The equilibrium constant in the gaseous system is Kp, it is expressed in terms of the partial…

Answered: (a) Formulate the equilibrium…

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 initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g), [NH3]i = 0.400 M, [N2]i = 0.155 M, [H2]i = 0.110 M, Kc = 16 What is the reaction quotient? What direction will the reaction shift to? (b) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g), Pi(NH3) = 2.10 atm, Pi(N2) = 10.70 atm, Pi(H2) = 10.70 atm, Kp = 8.3 ✕ 104 What is the reaction quotient? What direction will the reaction shift to? (c) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g), [SO3]i = 1.90 M, [SO2]i = 1.90 M, [O2]i = 1.90 M, Kc = 0.23 What is the reaction quotient? What direction will the reaction shift to? (d) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g), Pi(SO3) = 0.100 atm, Pi(SO2) =…
Balance each of the following examples of heterogeneousequilibria and write its reaction quotient, Q꜀:
11
In an experiment, gaseous C2H4 and H2O, at 25 mmol each, were mixed in a 50-mL flask that contains 2.5 mmol of C2H6. (a) Determine the equilibrium constant if, at equilibrium, 16 mmol of C2H6 was present. C2H4(g) + H2O(g) ⇋ C2H6(g) + O2(g) At one point of the experiment, it was found that 9.7 mmol C2H4, 7.5 mmol H2O, 21.9 mmol C2H6 and 16.4 mmol O2 were present in the flask. (b) At what direction should the reaction proceed to achieve equilibrium? Support your answer with calculations and explain your answer in not more than 3 sentences.
(a) (i) Define molar mass of a substance. (ii) State the method used to determine the molar mass of a volatile liquid. 2.15g ofa volatile liquid produced 84.3cm' of gas at 37°C and 0.97 atm. calculate the molar mass of the liquia. (iii) (b) (i) State the equilibrium law. TAG (ii) How will an increase in temperature affect the position of equilibrium of the reaction? N2O(g) = 2NO2(g) AH®=+54 kJ molľ Calculate the pH of an equivolume mixture of a 0.04 moldm® solution of CH3COOH and 0,3 moldm solution of CH3COONA (Ka = 2.0 x 10° moldm) (c) %3D
Which of the following stresses to a system at equilibrium cause an increase in the production of CH3OH ? CO(g)+ 2H2(g) → CH3OH(g) (a) H2 is added. (b) The volume is increased. (c) Argon is added. (d) Removing CO.
12.48 The following reaction is in equilibrium in lake water: HCO3(aq) + H+ (aq) = H₂CO3(aq) Predict the change in the reaction quotient, Q, for each disturbance below and use that prediction to explain how the equilibrium is shifted by the stress. (a) NaHCO3 is added to the lake. (b) H₂CO3 is added. (c) NaOH is added.
4. Consider an equilibrium mixture of the following chemical reaction : Fe"(aq) + SCN (aq) – Fe(SCN)³"(aq) yellow colourless deep red (a) Write an expression for the equilibrium constant Kc for the reaction. (b) At a certain temperature, the equilibrium constant Kc for the reaction is 1.08 x 10° dm³ mol1. The equilibrium mixture is prepared by mixing 20.0 cm³ of 0.030 M Fe(NO3)3(aq) with 10.0 cm³ of 0.030 M KSCN(aq) in an acidic medium. Calculate the concentration of Fe(SCN)²*(aq) in the equilibrium mixture at that temperature. (c) It is known that the equilibrium constant Kc increases when temperature increases. Suggest and explain whether the enthalpy change of the reaction is positive, negative or zero. (d) When a little amount of Na,SO3(s) is added to the equilibrium mixture, the colour of the mixture becomes paler. Explain this observation.
(b) At 100° C, the Keq for the Haber process is 4,51 X 10-5: N₂ + 3 H₂ 2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium (i) PNH3 105 atm, PN2 = 35 atm and PH2 = 495 atm (ii) PNH3 35 atm, PN2 = 0 atm and PH2 = 595 atm (iii) PNH3 = 26 atm, PN2 = 202 atm and PH2 = 42 atm (iv) PNH3 105 atm, PN2 = 5 atm and PH2 = 55 atm
(10). Subject :- Chemistry
2
Balance each of the following examples of heterogeneousequilibria and write its reaction quotient, Q꜀:

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