+O2 (8) 2 SO, (8) A,2.000 Lflask was initially filled with,0.0400 mol SO and 0.0200 mol O, and was allowed to reach equilibrium. If the flask contained, 0.0296 mol SO, at equilibrium: Consider the following: 2 SO, (e) 2 (g) 32 3. al Calculate the moles of each substance present at equilibrium. b| Calculate the equilibrium constant, K. + O2 (3) = 2SO, (8) 3 (g) c Calculate the equilibrium constant, K, for the following: 2 SO, +2O2(8) = 4 SO, (3) 2 (g) d| Calculate the equilibrium constant, K, for the following: 4 SO, (e) of HCN CHEMISTRY 1516L

+O2 (8) 2 SO, (8) A,2.000 Lflask was initially filled with,0.0400 mol SO and 0.0200 mol O, and was allowed to reach equilibrium. If the flask contained, 0.0296 mol SO, at equilibrium: Consider the following: 2 SO, (e) 2 (g) 32 3. al Calculate the moles of each substance present at equilibrium. b| Calculate the equilibrium constant, K. + O2 (3) = 2SO, (8) 3 (g) c Calculate the equilibrium constant, K, for the following: 2 SO, +2O2(8) = 4 SO, (3) 2 (g) d| Calculate the equilibrium constant, K, for the following: 4 SO, (e) of HCN CHEMISTRY 1516L

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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4. A. An important reaction in the commercial production of hydrogen is CO(g) + H2O(g) --><-- H2(g) + CO2(g) How will the system at equilibrium shift in each of the five following cases? (Use arrows or write "right" , "left" , or "no shift"). a. Gaseous carbon monoxide is removed b. In rigid reaction container, a catalyst is added. c. The temperature is decreased (the reaction is exothermic). d. The reaction container volume is doubled. e. Hydrogen gas is added. B. The equation above has a Kc value of 7.5 x 102. If 2.0 moles of each reactant and product are put into the same sealed 4.0 L container, determine the concentrations of all species present at equilibrium. Please answer A with sub parts and B.
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Question 12 of 50 Consider the equilibrium system described by the chemical reaction below. A 2.00 L reaction vessel was filled 0.0432 mol SO, and 0.0296 mol O, at 900 K and allow to react. At equilibrium, the concentration of SO, was found to be 0.0175 M. Determine the concentrations of all species at equilibrium and then calculate the value of Kc for this reaction. 2 SO,(g) + 0,(9) =2 S0,(g) 1 2 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. 2 SO,(g) 2 SO,(g) + (6)°o Initial (M) Change (M) Equilibrium (M) 5 RESET 2.00 0.0432 0.0296 0.0175 -0.0175 -0.0350 -0.00875 0.00875 0.0216 0.0148 0.0041 0.0129 0.0061 0.0257 0.0209 1L