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For the chemical equation SO, (g) + NO,(g) = S0;(g)+NO(g) the equilibrium constant at a certain temperature is 2.60. At this temperature, calculate the number of moles of NO,(g) that must be added to 3.36 mol SO,(g) in order to form 1.40 mol SO,(g) at equilibrium.

For the chemical equation SO, (g) + NO,(g) = S0;(g)+NO(g) the equilibrium constant at a certain temperature is 2.60. At this temperature, calculate the number of moles of NO,(g) that must be added to 3.36 mol SO,(g) in order to form 1.40 mol SO,(g) at equilibrium.

World of Chemistry, 3rd edition
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 39A
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This is my second time asking this question, the first one provided is incorrect.

For the chemical equation SO, (g) + NO, (g) = S0,(g)+NO(g) the equilibrium constant at a certain temperature is 2.60. At this temperature, calculate the number of moles of NO, (g) that must be added to 3.36 mol SO, (g) in order to form 1.40 mol SO,(g) at equilibrium. .224 moles of NO, (g): mol Incorrect
Transcribed Image Text:For the chemical equation SO, (g) + NO, (g) = S0,(g)+NO(g) the equilibrium constant at a certain temperature is 2.60. At this temperature, calculate the number of moles of NO, (g) that must be added to 3.36 mol SO, (g) in order to form 1.40 mol SO,(g) at equilibrium. .224 moles of NO, (g): mol Incorrect
Expert Solution Step 1 SO2(g)+NO2(g)----SO3(g)+NO(g) For the reaction, keg = [Product]/[Reactant] = [SO3][NO]/[SO2][NO2] %3D Keg = 2.6; [SO2] = 3.36 ; [SO3] = 1.4 = [NO] Step 2 [NO2] = [SO3][NO]/[SO2]keg = (1.4x1.4)/(3.36x2.6) = 0.224 mol
Transcribed Image Text:Expert Solution Step 1 SO2(g)+NO2(g)----SO3(g)+NO(g) For the reaction, keg = [Product]/[Reactant] = [SO3][NO]/[SO2][NO2] %3D Keg = 2.6; [SO2] = 3.36 ; [SO3] = 1.4 = [NO] Step 2 [NO2] = [SO3][NO]/[SO2]keg = (1.4x1.4)/(3.36x2.6) = 0.224 mol
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