zimjec@foxiomail.com Part AGiven the following reaction at 298 K:2 H2S(g) + SO2(g) → S8 (s) + 2 H20(g)Calculate A,G under the following conditions: PHS = 2.00 bar; Pso, = 0.165 bar; PH.0O = 1.164 barA‚G° = –102 kJ mol-1Express your answer using three significant figures and include the appropriate units.kJA‚G = -100molSubmitPrevious Answersv CorrectPart BIs this reaction more or less spontaneous than under standard conditions?The reaction is more spontaneous.The reaction is less spontaneous.SubmitPrevious Answersv CorrectPart CWhy?Under the nonstandard conditions the absolute value of the Gibbs energy change is smaller than under the standard conditions.Under the nonstandard conditions the absolute value of the Gibbs energy change is greater than under the standard conditions.Under the nonstandard conditions the Gibbs energy change is less positive than under the standard conditions.O Under the nonstandard conditions the Gibbs energy change is more positive than under the standard conditions.SubmitRequest AnswerO O O O

Under standard condition ΔGo=-102 kJ/mol Under non standard condition ΔG=-100 kJ/mol

• Part A Given the following reaction at 298 K: 2 H2S(g) + SO2(9) → Ss (s) + 2 H2O(9) Calculate A,G under the following conditions: P.s - 2.00 bar; Pso, =0.165 bar; P.0 = 1.164 bar A,G = -102 kJ mol Express your answer using three significant figures and include the appropriate units. 4,G. -100 kJ mol Previous Answers v Correct Part B Is this reaction more or less spontaneous than under standard conditions? The reaction is more spontaneous. • The reaction is less spontaneous. Submit Previous Answers v Correct Part C Why? O Under the nonstandard conditions the absolute value of the Gibbs energy change is smaller than under the standard conditions. O Under the nonstandard conditions the absolute value of the Gibbs energy change is greater than under the standard conditions. O Under the nonstandard conditions the Gibbs energy change is less positive than under the standard conditions. O Under the nonstandard conditions the Gibbs energy change is more positive than under the standard conditions. Submit Request Answer

• Part A Given the following reaction at 298 K: 2 H2S(g) + SO2(9) → Ss (s) + 2 H2O(9) Calculate A,G under the following conditions: P.s - 2.00 bar; Pso, =0.165 bar; P.0 = 1.164 bar A,G = -102 kJ mol Express your answer using three significant figures and include the appropriate units. 4,G. -100 kJ mol Previous Answers v Correct Part B Is this reaction more or less spontaneous than under standard conditions? The reaction is more spontaneous. • The reaction is less spontaneous. Submit Previous Answers v Correct Part C Why? O Under the nonstandard conditions the absolute value of the Gibbs energy change is smaller than under the standard conditions. O Under the nonstandard conditions the absolute value of the Gibbs energy change is greater than under the standard conditions. O Under the nonstandard conditions the Gibbs energy change is less positive than under the standard conditions. O Under the nonstandard conditions the Gibbs energy change is more positive than under the standard conditions. Submit Request Answer

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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