What is the rate law for the following mechanism: NO (g) + Br2 (g) 2 NOB12 (g) (fast equilibrium) (rate of forward reaction: k1, rate of reverse reaction: k.j) NOB12 (g) + NO (g) → 2 NOB1 (g) (slow, rate: k2) Rate= k2 [NOB12][NO] A. Rate= k1 [NO][Br2] OB. Rate= (k1/k.1) [NO][Br2] Rate= k2 (k1/k.j) [NOJ²[Br2] O E. Rate= k2 [NO]²{Br2]

MISSED THIS? Read Section 15.6 (Pages 656 - 661); Watch KCV 15.6, IWE 15.9. Consider this three-step mechanism for a reaction: 2Cl(g) (fast) HCl(g) +CC13 (g) (slow) (fast) Cl₂(g) k₂ Cl(g) + CHCl3 (g) → k₂ Cl(g) + CC13(g) → CCL (g) k₂ Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. ► View Available Hint(s) D_ | ΑΣΦ xa Xb a b a X → Submit Previous Answers A chemical reaction does not occur for this question. www X Incorrect; Try Again; 3 attempts remaining X ? P

A) In the proposed reaction mechanism below, the intermediate product is: A).  NO(g) B).  N2O2(g) C).  H2(g) D).  N2O(g)   B) The rate expression for a particular reaction is rate = k[A][B]^2. If the initial concentration of B is increased from 0.10M to 0.30M, the initial rate will increase by which of the following factors  A) 2 B) 3 C) 6 D) 9

A) Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3-  -->  4 Zn2+ + N2O(g) + 5 H2O(l) What is the rate law for this reaction? Group of answer choices rate = k [H+][NO3-] rate = k [H+]10[NO3-]2[Zn2+]4[N2O] More information is needed to determine this. rate = k [H+]10[NO3-]2   B) Consider the following reaction: 4 Zn(s) + 10 H+ + 2 NO3-  -->  4 Zn2+ + N2O(g) + 5 H2O(l) If the rate of H+ disappearance is 0.0250 M/min, what is the rate of Zn2+ appearance? Group of answer choices 0.0100 M/min 0.00100 M/min 0.0250 M/min 0.0625 M/min