Write the equilibrium constant expressions for K.and Kp, if applicable, for the following reactions:(a) 2NO2(8) + 7H2(8) = 2NH3(g) + 4H20(1)(b) 2ZnS(s) + 302(8) 2Zn0(s) + 2SO2(8)(c) C(s) + CO2(8) = 2C0(8)(d) C,HSCOOH(aq) =CH;CO0 (aq) + H*(aq)

In the given question we have to write the equilibrium constant for Kc and Kp of the following…

Answered: Write the equilibrium constant…

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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Write the equilibrium-constant, Kp, expression for the reaction A(g) + 4 B(1) = 3 C(g) + D(g) Answer Bank Kp = 3Pc PA 4 P3 P B
Consider a reaction A2(g) + B2(g)⇌2 AB(g), withatoms of A shown in red in the diagram and atoms of Bshown in blue. (a) If Kc = 1, which box represents the systemat equilibrium? (b) If Kc = 1, which box represents thesystem at Q < Kc? (c) Rank the boxes in order of increasingmagnitude of ΔG for the reaction.
For the following reaction: A(aq) + 2 B(ag) = 2 C(ag) + 2 D(ag) Calculate the magnitude of Ke (don't report the units) assuming the following composition at equilibrium: [A] = 0.339 mol L-1 [B] = 0.864 mol L-1 [C] = 0.476 mol L-1 [D] = 0.163 mol L-1 %3D
1. NO2(g) and N₂O4(g) are in a reaction vessel with partial pressures 0.510 bar and 0.800 bar respectively. A,Gº = -2.80 kJ mol-¹. Is this system at equilibrium at 298 K? (a) Yes (b) No
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Be sure to answer all parts. The equilibrium constant for the reaction AS B is K.= = 10 at a certain temperature. (1) Starting with only reactant A, which of the diagrams shown below best represents the system at equilibrium? The gray spheres represent the A molecules and the green spheres represent the B molecules. (a) (b) (c) (d) (a) (b) (c) (d) (2) Which of the diagrams shown above best represents the system at equilibrium if K. = 0.10? (a) (b) (c) (d)
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The equilibrium constant, Kc, for the following reaction is 1.29x10-2 at 600 K. coCI,(g) ? CO(g) + Cl2(g) Calculate the equilibrium concentrations of reactant and products when 0.373 moles of COCI2(g) are introduced into a 1.00 L vessel at 600 K. [COCI2] = [CO] M [Cl2] M ΣΣΣ
Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375 X (b) What is Kp if the total pressure is 10.5 atm? 9.12
Use the data in the supporting materials to calculate the equilibrium constant (Kp) for the following reaction at 25°C. 2 SO2(g) + O2(g) =2 S03(g) Кра 4.24e24 Calculate Kp for the reaction at 49°C using the following equations. (a) the van't Hoff equation below. (P), A,H° RT? a In K Кр = 1.138e22 (b) the Gibbs-Helmholtz equations below to find A-G° at 49°C and hence, Kp at the same temperature. AG ΔΗ (i) = - T2 A-G2 A;G1 1 (ii) T2 T1 T1 Kp = 1.138e22 (c) A-G° = ArH° – TA¡S° to find A-G° at 49°C and hence, Kp at the same temperature. Кр 3D 1.7742е22 State the approximations employed in each case. The assumption that A,H° is temperature independent and equal to the value calculated at 298.15 K is required by all three parts A second assumption that AS° is temperature independent and equal to the value calculated at 298.15 K is required by part (c) Compare your results. The answers calculated in parts (a) and (b) ▼ in part (c) are very close as expected because the formulas used to…
Use the References to access important values if needed for this question. The equilibrium constant in terms of pressures for the reaction C,H;CH,OH(g)=C,H;CHO(g) + H2(g) is K, = 0.558 at 523 K. (a) A pure sample of gaseous benzyl alcohol, C,H¿CH,OH(g), is introduced into a rigid flask at a temperature of 523 K so that its original pressure is 0.132 atm. Calculate the fraction of this starting material that is converted to products at equilibrium. (b) A second sample of benzyl alcohol is introduced into a rigid flask at a temperature of 523 K, this time at an original pressure of 4.14 atm. Again, calculate the fraction of the starting material that is converted to products at equilibrium.

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Write the equilibrium constant expressions for K. and Kp, if applicable, for the following reactions: (a) 2NO2(8) + 7H2(8) = 2NH3(8) + 4H20(1) (b) 2ZnS(s) + 302(8) 2Zn0(s) + 2SO2(8) (c) C(s) + CO2(8) (d) C,HSCOOH(aq) = = 2C0(g) CH;CO0 (aq) + H* (aq)