Question

< Week 2 Assignment: Nuclear Chemistry and Chemical Equilibrium Equilibrium Constant and Reaction Quotient 16 of 36 > Review Constants Periodic Table At equilibrium, the concentrations of reactants and products can be predicted using the equilibrium constant, which is a mathematical expression based on the chemical equation. For example, in the reaction A+BBC + dD Part A where a, b, c, and d are the stoichiometria coefficients, the equilibrium constant is A mixture initially contains A, B, and in the following concentrations: A -0.650 M B - 1.00 M, and C -0.600 M. The following reaction occurs and equilibrium is established: A + 2B At equilibrium, (A) - 0.550 M and C -0.700 M. Calculate the value of the equilibrium constant, Express your answer numerically. View Available Hint(e) KD IA"B" where (A). (B) (C), and [D] are the equilibrium concentrations. If the reaction is not al equilibrium, the quantity can still be calculated, but it is called the reaction quotient, Q. Instead of the equilibrium constant, K. 80 AED ROm ? Q = D K- (ALBL where each concentration is measured at some arbitrary time t. Submit Part B Complete previous part(s)

Answer 1

Initial concentration of A = 0.650 M Initial concentration of B = 1.00 M. Initial concentration of C = 0.600 M Let x be the change in the concentration of each species at equilibrium. Kc M 1A + 2B Initial 0.650 1.00 0.600 change -X - 2x + x equilibrium 0.650 - X 1.00 - 2x 0.600 + x At equilibrium, concentration. of A= 0.550 M That is 0.650- x = 0.216 So, x = 0.650 - 0.550 = 0.100 M Equilibrium concentration of A = 0.650 M Equilibrium concentration of B = 1.00 – 2x = 1.00 – 2(0.100) = 0.800 M Equilibrium concentration of C =0.700 The equilibrium constant is given by K = [C] [4][B] (0.700) K =1.988636 =1.99 (0.550)(0.800) K=1.99