part b please Assuming ideal gas behavior, calculate the mass of H2 (in g) present in the reactionmixture at equilibrium.Hydrogen can be extracted from natural gasaccording to the following reaction:CH4 (g) + CO2 (9) = 2 CO (g) + 2 H2 (g)K, = 4.5 × 10² at 825 KAn 85.0-L reaction container initially contains 22.3kg of CH4 and 55.4 kg of CO2 at 825 K.365 gSubmitPrevious Answersv CorrectPart BWhat is the percent yield of the reaction under these conditions?ΑΣφ?0%

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Assuming ideal gas behavior, calculate the mass of H2 (in g) present in the reaction mixture at equilibrium. Hydrogen can be extracted from natural gas according to the following reaction: CHa (9) + CO2 (9) — 2 СО (9) + 2 H2 (9) К, — 4.5 х 10? at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. 365 g Submit Previous Answers v Correct Part B What is the percent yield of the reaction under these conditions?

Assuming ideal gas behavior, calculate the mass of H2 (in g) present in the reaction mixture at equilibrium. Hydrogen can be extracted from natural gas according to the following reaction: CHa (9) + CO2 (9) — 2 СО (9) + 2 H2 (9) К, — 4.5 х 10? at 825 K An 85.0-L reaction container initially contains 22.3 kg of CH4 and 55.4 kg of CO2 at 825 K. 365 g Submit Previous Answers v Correct Part B What is the percent yield of the reaction under these conditions?

World of Chemistry, 3rd edition

3rd Edition

ISBN:9781133109655

Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 34A

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