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: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 81QAP

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5a-please see attached
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