1. A proposed mechanism for a reaction is as below: Step 1: C4H:Br → C4H9* + Br Step 2: C4H + H:0 > САНООН* Step 3: C:H9OH+ + H2O –→ C:H9OH + HsO* (slow) (fast) (fast) (a)What is the overall balanced equation for the reaction? (b) Identify any intermediates in the proposed mechanism. (c) Write the rate law expected for this mechanism.

For the reaction: 4NH3 (g) + 7O2 (g) → 4NO2 (g) + 6H2 (g), if H2 is produced at a rate of 3.5 x 10-3 M/s, O2 is consumed at a rate of... A. -2.5 x 10-2 M/s B. -4.1 x 10-3 M/s C. -2.1 x 10-2 M/s D. -3.0 x 10-3 M/s E. -5.8 x 10-4 M/s

Assignment 1. The reaction 2NO (g) t CL (g) 2NOCI (g) was studied at- 10 C. The following results were obtained where Rate =- A[CI1 At [2NO], (mol / L) (Ch], (mol/L) Initial Rate (mol /L min) 0.18 0.10 0.10 0.10 0.20 0.36 0.20 0.20 145 a) What is the rate law b) What is the value of the rate constant

How much time does it take to reduce the concentration of NO2 by half by looking at the reaction process curve below?

1.a) For the reaction below, A[HBr]/At = 5.0 x 10-5 M/s. What is the rate of formation of Br2 ? 2 HBr(g) > Br,(g) + H2(g) а. 5.0 x 10-5 M/s b. 2.5 х 10-5 М/s с. 1.0 х 10-4 Ms d. 1.0 x 10-5 M/s 1b) Assume that you doubled the concentration of HBr in the previous problem and the rate increased by a factor of 4. What would be the rate law for this reaction? a. rate = k[HBr] b. rate = k[HBr]? c. rate = k[HBr]4 d. rate=[Br2][H2]/[HBr]?

= ○ KINETICS AND EQUILIBRIUM Expressing the concentration of an intermediate in terms of the... Consider the following elementary reaction: CFC1₂(g) → CFC1₂(g) +C1(g) Suppose we let k₁ stand for the rate constant of this reaction, and k_₁ stand for the rate constant of the reverse reaction. 1 Write an expression that gives the equilibrium concentration of CFC1, in terms of k₁, k₁, and the equilibrium concentrations of CFC13 and C1. 1' [CFC₁₂] = 0 √6 X 5 0/5

03+0 --> 202 Nitrogen oxide (NO) in the atmosphere can react with ozone as well according to the following steps: NO + O3 --> NO2 + O2 NO₂+O--> NO + O₂ 1) What is the overall reaction that results from NO reacting with ozone? 2) Identify any catalysts in the reaction. If there are none, write none. 3) Identify any intermediates in the reaction. If there are none, write none.

The kinetic data shown below were observed for the reaction:    BF3 (g)     +   NH3 (g)    --------->      F3B·NH3 (g)   Trial # [BF3] (mol/L) [NH3] (mol/L) Rate (M/s) 1 0.250 0.250 0.2130 2 0.250 0.125 0.1065 3 0.200 0.100 0.0682 4 0.350 0.100 0.1193 5 0.175 0.100 0.0596 What is the rate constant for this experiment?

Use this data for the following four (4) questions: The relative initial rates of the reaction A2 + B2-products in vessels (a)-(d) are 1:1:4:4. The spheres represent the number of molecules of present at the beginning of the reaction. [Unshaded spheres = A2 molecules; shaded spheres = B2 molecules] %3D For example, vessel (a) contains 2 A2 molecules and 2 B2 at the beginning of the reaction. Rate = 1 Rate 1 Rate = 4 Rate = 4 %3D 2. 8. 80 (c) (a) 11) What is the order of reaction with respect to A2? (b) (d) BA 11) A))0 B) 1 C) 2 D) 3 12) What is the order of reaction with respect to B2? 12) C A) 0 B) 1 D) 3 13) o c 13) What is the overall order of reaction? A) 0 B) 1 D) B 14) 14) What is the rate law for this reaction? B) Rate k[B2]2 D) Rate = k[A2]2[B2]² A) Rate = k[A2]² %3D C) Rate = k[A2][B2] %3D %3D nation below: 15) 8. 8.

Consider the reaction 2 D(g) + 3 E(g) + F(g) → 2 G(g) + H(g). When [E] is decreasing at 0.10 mol/ L-s, how fast is [D] decreasing? (Disregard the use of any negative sign.) 0.30 mol/ L-s 0.15 mol/ L-s None of these 0.10 mol/ L-s 0.067 mol/ Ls