Problem Set 5. The gas-phase decomposition of N₂O is believed to occur via two elementary steps: Step 1: N₂O → N₂ + O 2 Step 2: N₂O + 0 ➜ N₂ + O₂ 2 k₁ 1 k₂ Experimentally, the rate law is found to be rate=k[N₂O]. a. Write the equation for the overall reaction. b. Identify the intermediate. c. What can you say about the relative rates of steps 1 and 2? 1-1

2. What is the rate law for the theoretical reaction 2 A + B C + 2 D? a. rate = K[A]² [B] b. It is impossible to determine from this information. c. rate= K[C][D]² d. rate = k[A][B]

You have a reaction: A + B --> C The reaction is first order with respect to A and 2nd order with respect to B. If 1.3 mol of A is mixed with 2.3 mol of B to make a 1.000 L solution and the rate of the reaction is 1.6 M/s, what is the rate constant (k)?

A certain chemical reaction 2A → B + C is proposed to occur in three elementary steps:    Step 1:   A  ⇌  B + D   (fast)    Step 2:   D  ⇌  E   (slow)    Step 3:   A + E  →  C   (fast) Which one of the following rate laws is consistent with the proposed mechanism?   A.  Rate = k[A][B]–1   B.  Rate = k[A]2   C.  Rate = k[A]3[B]–1   D.  Rate = k[A]2[B]–1   E.  Rate = k[A]