The following mechanism has Proposed for the reaction of A with E: Step 1: A + E
ID: 959977 • Letter: T
Question
The following mechanism has Proposed for the reaction of A with E: Step 1: A + E rightarrow C + D (slow) Step 2: C + E rightarrow B + D Write the equation for the overall reaction. Identify any intermediate in the mechanism. What is the rate law of the overall reaction. if the first reaction happens slower than the second action? Write the equilibrium-constant expression K for the following reactions: Cd^2+ (aq) + 4 Br (aq) CdBr_4^2- (aq) MgCO_3(s) 3 Fe (s) + 4 H_2O (g) Fe_3O_4(s) + 4 H_2 (g) CO_3^2- (aq) + H_2O (I) OH^- (aq) + HCO_3^- (aq) An aqueous solution of acetic acid is found to have the following equilibrium concentrations at 25 degree C: [CH_3COOH] = 1.65 times 10^-2 M; [H^+] = 5.44 times 10^-4 M; and [CH_3COO^-] = 5.44 times 10^-4 M. Calculate the equilibrium constant K. for the ionization of acetic acid at 25 degree C. The reaction is CH_3COOH(aq) H^+(aq) + CH_3COO^-(aq) Equilibrium partial pressures of NOCI, NO, and Cl_2 in a container at 300 K are 1.2 atm. 0.050 atm. and 0.30 atm. respectively, (a) Calculate the equilibrium constant K_p for the reaction 2 NO (g) + Cl_2 (g) 2 NOCl(g). (b) Calculate K_c for this reaction at this temperature. (R = 0.08206 L.atom/mol-K) Given that at 700 K, K_p = 54.0 for the reaction H_2 (g) + I_2(g) 2 HI (g) and K_p = 1.04 times 10^-4 for the reaction N-2 (g) + 3 H_2 (g) 2 NH_3 (g), determine the value of K_p at 700 K for the reaction 2 NH_3 (g) + 3 I_2(g) 6 HI (g) + N_2 (g)Explanation / Answer
9
a)
overall rreaction
1 + 2
A + E + C + E = C + D + B + D
cancel common terms
A + 2E = B + 2D
b)
intermediate are those that not appear in the overall reaction
in this case "C"
c)
choose the determinant step, which is th eslower
then
A+E = C+D
Rate = K*[A][E]
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