31. Listed below are AH; and S° values for PCI 3, Cl2, and PCl5.SubstanceAH (kJ mol¹)So (J.mol-1.K-1)PC13 (g)-287311.8C12 (9)0223.1PCl5 (g)-374.9364.6Use these data to calculate the equilibrium constant (Keq) for the formation of PCl5 (g) from PC|3(g) and Cl2 (g) at 200.0°C, as shown below.A.0.137B.0.155C.3.98D.6.43E.7.32PC13 (g) + Cl2 (g) = PCl5 (g)

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Answered: 31. Listed below are AH; and S° values…

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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At -9.76 °C the concentration equilibrium constant K = 5.3 × 105 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 11.%. • If the reaction is run at constant pressure, 64.0 kJ/mol of heat are released. • The net change in moles of gases is - 1. Using these facts, can you calculate K at 15. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether K at 15. °C will be bigger or smaller than K at -9.76 °C? O Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. O No. 0 x10 X
0. A 3.73 kg cast iron pan is heated to 824 °C and subsequently quenched in 2.0 gallons (approximately 7.57 L) of mineral oil at 20.0 °C to harden the cast iron. The system is , lowed to reach equilibrium. What is the temperature (in °C) of the system at equilibrium? (Cs,iron = 0.460 J g°C-; Cs,oil = 1.67 J g¬1 °C-1; don = 0.850 g mL-) %3D %3D A: 131
HCO2H? Material from chapter 12, 15 2 NO2 (g) > N2O4 (g) AH = -57.23 kJ/mol a. Is this endothermic or exothermic? b. If 5 mols of NO2 react, what is the amount of energy absorbed? What intermolecular forces are present in NO2 (g)? С. d. Write the equilibrium constant expression. How does the equilibrium shift i. as the temperature is increased? ii. as more N2O4 (g) is added? iii. as the volume is decreased? e.
26) Suppose that at a pressure of 1 atm and temperature 300 K, a given material has two possible phases: liquid (L) and solid (S). We start the system with N₁ = 5 moles in the liquid phase and Ng = 9 moles in the solid phase. For these values of pressure and temperature, PL = 5 x 10-21 J • Hs9 x 10-21 J. What is the equilibrium value of NL? a. 9 mol b. 14 mol c. 1.49 mol d. 5 mol e. O mol
2 CO₂ (g) = 2 CO (g) + O₂ (g) 1. Write the K. expression for this balanced equation. 2. If, at equilibrium, the concentrations of the reactants and products are as follows: [CO] = 0.00025 M, [0₂] = 0.00050, [CO₂] = 0.25 M, calculate the value for Kc. 3. Where does the equilibrium lie, towards the products or reactants? How can you know?
ient/takeCovalentActivity.do?locator-assignment-take Consider the following system at equilibrium where AH° = 198 kJ, and K. = 2.90x102, at 1.15x10° K. 2S03(g) 2S02(g) + O2(g) If the VOLUME of the equilibrium system is suddenly increased at constant temperature: The value ofK. A. increases. B. decreases. C. remains the same. The value of Q. A. is greater than K.. B. is equal to K. C. is less than K. The reaction must: A. run in the forward direction to reestablish equilibrium. B. run in the reverse direction to reestablish equilibrium. C. remain the same. It is already at equilibrium. The number of moles of O, will: A. increase. B. decrease. C. remain the same. Submit Answer Retry Entire Group 8 more group attempts remaining Prev

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