105. Mechanism of NO, Destruction Which of the following mechanisms are possible for the thermal decomposition of k[NO3]? NO2, given that the rate = slow → NO(g) + O(g) NO(g) + O2(g) NO;(g) a. fast O(g) + NO2(g) b. NO2(g) + NO,(g) fast → N2O4(g) slow NO(g) + NO3(g) NO(g) + O2(g) NO(g) + NO3(g) NO(g) + O2(g) N,O.(g) NO3(g) fast slow c. NO2(g) + NO;(g) NO3(g fast ,

Consider the following reaction mechanism: Step 1: 2NO (g) + 1.50,(g) --> N,Og(s) Step 2: 2NO,(g) --> 2NO(g) + O2 (g) Write the overall reaction and identify any reaction intermediates.

The variation of the rate constant with temperature for the decomposition of HI(g) to H2(g) and I2(g) is given here. What is the activation energy for the reaction?                                                2HI(g) ⟶ H2(g) + I2(g)

Nitrosyl chloride, NOCL decomposes to NO and Cl Determine the reaction arder with respect to NOCI from the following data: 2NOCI 2NO + Clz NOCIJ (M) 0.10 0.20 0.30 Rate (mol Lh) 8.0 x10 10 3.2 x10 72x10 O frst onder O second onder O hird onder

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

3. Consider NO₂ (g) + CO (g) → NO (g) + CO₂ (g). The initial rates are shown in the table below. Please compute (a) the rate law for the reaction and (b) compute the value of k. [CO] 0.050 0.050 0.100 0.100 [NO₂] 0.050 0.100 0.200 0.100 Initial Rate (M/s) 0.0040 0.016 0.256 0.0640

The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.

59.)

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)?

4. Ammonium nitrite, NHẠNO2, decomposes in solution as shown: NHẠNO2 (aq) N2(g) + 2H20(1) The concentration of NH,* ion at the beginning of the experiment was 0.500M. After 3 hours, it was 0.432 M. What is the average rate of decomposition of NHẠNO2 in this time interval?