Question

CHE 1314 Exam 3-Version A-Spring 2019 Dr. Brown 16. Consider the reaction and the initial concentrations given below. Is the reaction at equilibriumi? (8) If not, then which way will the reaction proceed (left or right) to attain equilbrium? Initial: [0.45] [0.20](0.70] 015-x 0 200 701x 0 120 The reaction below has a Kc 14.32. The equilibrium concentration of N204 was found to be 0.8905 M. Calculate the equilibrium concentration of NO2. 17. (8) 0.8105 N201 N2041 4
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Answer 1

Consider the reaction and initial concentrations given below Is the reaction at equilibrium ? IF not, men which way will me reaction proceed (left or right) to equilibrium 2H_2 (g) + O_2(g) rightleftharpoons 2H_2(g) kc = 0.726 Initial [0.20] [0.70] doublerightarrow Given value k_c = 0.726 To determine the direction of the reaction we need to determine Q_c (reaction Quotient) it can be determined at any instant of time but k_c me equilibrium constant * If Q_c - k_c the reaction is at equilibrium * If Q_c > k_c the reaction is favored in reverse direction (or) constant direction i e the reaction proceeds to left *If Q_c < k_c the reaction is favored in forward direction (or) The reaction proceeds to right Based on given values i e [H_2] = 0.45 [O_2] = 0.20 Q_C = [H_2O]^2/[H_2]^2 [O_2] Q_c = (0.70)^2/(o.45)^2 (0.20) Q-c = 12.099