2. Consider a closed vessel containing a mixture of ideal gases A and B thatundergo the chemical reaction:A=bB,where b is an unknown stoichiometric coefficient. The equilibrium mole fractionxд is measured but xB is unknown.The equilibrium mole fraction xд increases when the temperature in the vesselis increased with the pressure held constant and Ꮖ Ꭺdecreases when the pressurein vessel is increased with the temperature held constant.Explain these observations in terms of inequalities involving the enthalpy ofreaction AH and the stoichiometric coefficient b in Eq. (7).

To explain the observations in terms of inequalities involving the enthalpy of the reaction (ΔH) and…

Answered: 2. Consider a closed vessel containing…

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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Provide the formal definition of enthalpy and explain all symbols used in it. Explain how the change in enthalpy is related to certain thermodynamic property (other than Gibbs energy).
Consider the equilibrium system described by the chemical reaction below. Calculate the value of Qc for the initial set reaction conditions in 2.50 L container: 11.1 g C, 2.45 g H:O, 15.3 g CO and 7.55 g H2. C(s) + H:O(g) = CO(g) + Ha(g) Based on the given data, set up the expression for Qc and then evaluate it. Do not combine or simplify terms. Qc =
For the reaction 3H2(g)+N2(g)⇌2NH3(g) at 225 ∘C the equilibrium contant is 1.7×10 ^2. If the equilibrium mixture contains 0.19 M H2 and 0.015 M N2, what is the molar concentration of NH3? Express your answer to two significant figures and include the appropriate units.
Consider the following reaction that has a Kc = 2.4 x 10^-3 at 1000K: N2(g) + 3 H2(g) = 2NH3(g) in a reaction vessel that is 5.0 x 10^3 L, 250 moles of N2, 250 mol of H2, and 50.0 mol of NH3 are mixed. write the reaction quotient. Calculate Qc.
For the following reaction: A(g) + B(g) = 2 C(a) Calculate the magnitude of K, (don't report the units) assuming the following composition at equilibrium: PA = 0.438 bar PB = 0.716 bar Pc = 0.122 bar
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) =…
For the following reaction: A(g) + 3 B(g) magnitude of Kp (don't report the units) assuming the following composition at equilibrium: PA = 0.735 bar PB = 0.603 bar Pc = 0.627 bar PD 0.87 bar = 2 C(g) + D(g) Calculate the =
For the equilibrium reaction. 2IBr (g) I2 (g) + Br2 (g) Kc=.0085. If .025 M of IBr is introduced to an empty flask and allowed to reach equilibrium, calculate the final concentrations of all components. Consider the decomposition reaction at 555 K 4POCl3 (g) P4 (g) + 2O2 (g) + 6Cl2 (g) If .450 atm of POCl3 is introduced to an otherwise empty flask and the reaction is allowed to reach equilibrium, the final total pressure is .850 atm. Find Kp and Kc.
Consider the reaction: Nio (s) + CO (9) = Ni (s) + CO2 (g) K. =4000.0 at 1500 K When calculating the answer, do not round to the appropriate number of significant figures until the last calculation step.
Calculate the reaction quotient, Qr for the following reactions and conditions: 7. 2 SO3(g) 2 SO2(g) + O2(g) 16.5; Pso3 = 0.45 atm; Pso2 = 1.52 atm; : Кр- %3D Po2 = 0.210 atm 8. 2 NO(g) + Cl2(g) → 2 NOCI(g) : Кр- 2.5 x 103; PNo = 0.0032 atm; Pc12 = 0.023 atm; PNOCI = 0.210 atm 9.2 NH3(g) N2(g) + 3H2(g) : Кр- 17.0; PNH3 = 0.13 atm; PN2 = 0.34 atm; |3D PH2 = 1.1 atm %3D 10. Will the system in Question 7 proceed to reactants or products for the conditions given? 11. Will the system in Question 8 proceed to reactants or products for the conditions given? 12. Will the system in Question 9 proceed to reactants or products for the conditions given? 13. For the chemical reaction in Question 7, if it is at equilibrium which direction will it shift if SO2 is added? 14. For the chemical reaction in Question 8, if it is at equilibrium which direction will it shift if NO is removed? 15. For the chemical reaction in Question 9, if it is at equilibrium, which direction will if shift if all the…

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