me rate law for the reaction NH(aq) + NO2(aq) - ► N₂ (g) + 2 H₂O (1) given by rate = | = k[NH][NO]./ 1 At a certain temperature, the rate constant is 4.40 × 10-4 M-s alculate the rate of the reaction at that temperature if [NH] = = 0.261 M and [NO2] = gits. = 0.210 M. Be sure your answer has the correct number of significant

4) Use the data below to determine the rate law and the value of k for the following reaction CHC13 (g) + Cl2 (9) → CC14 (g) + HCl (g) [CHCI3] (M) [Cl2] (M) Initial Rate 0.0035 Experiment 1 0.010 0.010 2 0.020 0.010 0.0069 3 0.020 0.020 0.0098 4 0.040 0.040 0.0270

The reaction described by H, (g) + 1,(g) → 2 HI(g) has an experimentally determined rate law of rate = k [H2][I2] Some proposed mechanisms for this reaction are: Mechanism A (1) H, (g) + L,(g) 2 HI(g) (one-step reaction) Mechanism B (1) 1,(g) =2 1(g) (fast, equilibrium) k_1 (2) H, (g) + 2 I(g) –→ 2 HI(g) (slow) Mechanism C (1) I, (g) = 2 I(g) (fast, equilibrium) k_ k, (2) I(g) + H, (g) –→ HI(g)+H(g) (slow) (3) H(g)+I(g) → HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? O mechanism A O mechanism B O mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an I, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? O mechanism B O mechanism C O mechanism A

8. (15 marks) A reaction is written as A(g) At 298 K, k₁ =0.21 s.1. k.₁=5×10 Pa¹·s¹. B(g) + C(g). k-1 As the temperature increased from 298 K to 310 K, the values of k₁ and k., are doubled (denoted as k2 and K.2). (1) Calculate the rate constant k at 298K; (2) Calculate the activation energy of both forward and reverse reactions; (3) Calculate AH and AU for the reaction at 298K; (4) Calculate the reaction time at the whole pressure reaching to 152 kPa. The initial pressure of A(g) is 100 kPa and the reaction temperature is 298 K.