3. The equilibrium constant for the reaction:250:(g) + O:(g) = 2so:(g)is 2.8 x 10° at 25.0°c.a. Determine the Free Gibb's Energy in kJ/mol.b. Using the data provided below, determine the enthalpy of reaction (kJ/mol) and entropy ofreaction (J/mol K)SubstanceSO:(g)0:(g)SO:(g)AH; (kl/mol)S U/Kmol)c. Determine the entropy for the surroundings in J/mol K at 25.0°C.-296.4-395.2248.5205.0256.2d. Determine the entropy of the universe in J/mol K at 25.0°C.e. Is the reaction spontaneous at 25.0°C? Explain your answer using the information calculatedin part a and part d.

Given, reaction : 2SO2(g) +O2(g)⇌2SO3(g) Equilibrium constant , Keq=2.8×102

3. The equilibrium constant for the reaction: 250:(8) + O:(8) = 250,(8) is 2.8 x 10' at 25.0°C. a. Determine the Free Gibb's Energy in kJ/mol. b. Using the data provided below, determine the enthalpy of reaction (kJ/mol) and entropy of reaction (J/mol K) Substance AH, (k]/mol) S'(J/Kmol) c. Determine the entropy for the surroundings in J/mol K at 25.0°C. |SO:(g) -296.4 | 0:(8). SO(g) -395.2 248.5 205.0 256.2 d. Determine the entropy of the universe in J/mol K at 25.0°C. e. Is the reaction spontaneous at 25.0°C? Explain your answer using the information calculated in part a and part d.

3. The equilibrium constant for the reaction: 250:(8) + O:(8) = 250,(8) is 2.8 x 10' at 25.0°C. a. Determine the Free Gibb's Energy in kJ/mol. b. Using the data provided below, determine the enthalpy of reaction (kJ/mol) and entropy of reaction (J/mol K) Substance AH, (k]/mol) S'(J/Kmol) c. Determine the entropy for the surroundings in J/mol K at 25.0°C. |SO:(g) -296.4 | 0:(8). SO(g) -395.2 248.5 205.0 256.2 d. Determine the entropy of the universe in J/mol K at 25.0°C. e. Is the reaction spontaneous at 25.0°C? Explain your answer using the information calculated in part a and part d.

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...

See similar textbooks

Similar questions

Use thermodynamic values in the table provided to calculate the ΔG for the following process in two ways. 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) at 25˚C a) Use Free Energy values to calculate ΔG. b) Use Enthalpy and Entropy values with Gibbs Equation to calculate ΔG. c) What do your final ΔG values tell us about this reaction?
Consider the reaction Cl,(g) + Br,(g) 2 BrCl(g) at 25 °C. The entropy change for the reaction is 11.6 J/mol· K. If the standard enthalpy change is 29.4 kJ/mol for the reaction, then what is the standard free energy for the reaction? |kJ/mol 4 6. C 7 9. +/- х 100 +
5. Consider the combustion reaction of octane (C8H18, mol. wt. = 114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. 2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O b. Calculate the standard free energy (in kJ/mol) released in this reaction. ∆Hfo (kJ/mol) Sfo (J/K mol) Octane(l) ─208.4 463.7 H2O(g) ─242 189 02 0 205 CO2(g) ─393.5 214 c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts)
What is the free energy change for the following reaction at 25 oC if the entropy change at this temperature is - 10 J/molK? 3 A (g) + B (s) ------ 2 C (g) + 3.40 kJ A. - 3.30 kJ/mol B. + 6.38 kJ/mol C. + 0.420 kJ/mol D. - 6.38 kJ/mol E. - 0.420 kJ/mol
Benzene is a liquid under standard conditions. The standard enthalpy and entropy changes for the evaporation of liquid benzene to form benzene vapor are +33.9 kJ/mol and 96.3 J/mol · K, respectively. If liquid benzene is placed in a closed container at 78.85°C, which of the following statements is true? The liquid cannot attain equilibrium with its vapor in a closed container. a. b. The liquid will evaporate completely. Liquid benzene will evaporate until the vapor pressure is 1 bar. d. Liquid benzene will not evaporate. e. Liquid and vapor-phase benzene cannot coexist at temperatures greater than or equal to 78.85°C.
This reaction is _______ (product or reactant) favored under standard conditions at 330 K
Calculate the standard entropy, ASixn, of the reaction at 25.0 °C using the table of thermodynamic properties. 3 C,H, (g) C,H,(1) ASixn J-K-l.mol-1 Calculate the standard Gibbs free energy of the reaction, AGxn. The standard enthalpy of the reaction, AHxn, is -633.1 kJ-mol-1. AGixn kJ-mol-1 Determine in which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. forward reverse neither both
None
The decomposition of crystalline N2O5N2O5(s)?2NO2(g)+12O(g)is an example of a reaction that is thermodynamically favored even though it absorbs heat. At 25 ?C we have the following values for the standard state enthalpy and free energy changes of the reaction: Delta H = +109.6 kJ/mol Delta Standard Gibbs Free Energy = -30.5 kJ/mol C) Calculate delta U for this reaction at 25 C.