the reaction N2+3H2 arrow 2NH3, the rate of consumption of H2 was observed to be 3.50x 10^-4 M/s under certain conditions.  a. determine the rate of production of ammonia. b. determine the rate of this reaction.

6. The rate law for the overall reaction 2 N2O5 (g) →4 NO2 (g) + O2 (g) is Rate = k[N2O5). a. Consider this mechanism: i. N2O5 (g) → NO: (g) + NO2 (g) ii. NO2 (g) + N2Os (g) →3 NO2 (g) + O2 (g) i. NO: (g) +0 (g) → NO2 (g) + O2 (g) Is this reaction mechanism consistent with the rate law? Why or Why not? [fast) [slow] [fast] b. If the reacuion mechanism is not consistent with the rate law, how would it need to change to become consistent? c. List potential reaction intermediates present in uNIS nechanism d. Draw a reaction energy diagram for this mechanism including any modifications you've made in a-c.

4. Consider the following 3 step reaction mechanism: Step 1 H₂ 2H fast Step 2 Step 3 H + HCO H + CO a. What is the overall reaction? HCO slow H₂CO fast b. Identify the intermediates in the reaction mechanism. c. Write a rate law expression for each step of the mechanism including any reversible reactions. c. What is the predicted rate law expression? Be sure to only list reactants from the overall equation and not intermediates in the rate law expression.

2. Here are representations of a reaction: A + B> products Unshaded spheres represent A molecules. Shaded spheres represent B molecules. Trial 1 Trial 2 Trial 3 Trial 4 Rate = 1 Rate = 1 Rate = 4 Rate = 4 a. What is the order with respect to A (unshaded)? Explain how you determined this. b. What is the order with respect to B (shaded)? Explain how you determined this. c. What is the rate equation for this reaction? Explain how you determined this.

What would happen to the rate of a reaction with rate law rate = k[NO]<[H,] if the concentration of H, were halved? O A. The rate would not change. O B. The rate would be doubled. O C. The rate would be four times larger. O D. The rate would also be halved.

2. At low temperatures the rate law for the reaction (½ A+ ½ B → C) is - r₁ =k₁ C₁ CB. If the reaction is reversible at high temperatures, what is the rate law?

1. write a basic form of the rate law for the following reaction. NO-3 + 3I- + 2H+ ------> NO-2 + I-3 + H2O 2. if doubling the concentration of nitrate ion in the reaction above causes the rate of reaction to quadruple, what is the order of reaction with respect to nitrate ion?

a. Calculate the average rate of the reaction A to B from the start of the reaction to the 10th sec. b. Calculate the average rate of the reaction A to B between 10th sec and 20th sec. c. Which of the following statements about the reaction A B must correct?A. [A] = 0.025 M when time = 30 sec.B. At the end of reaction, [B] = 0.20 M.C. The rate of reaction decreases with time.D. [A] = [B] when time = 10 sec.

4. What is the value of x, the order of the reaction with respect to [OH']? k'/k" = (1/0.5)* 5. What is the value for the rate constant, k? k= k'/1* = %3D k =k"/0.5*= SaD 6.

Draw tructu f he ajor rganic roduct f he ollowing reaction. CH2 1. Hg(OAc)2, H20 2. NaBH4 CH3 • In cases where there is more than one answer, just draw one. •You do not have to consider stereochemistry. [ド