The decomposition of N205 in solution in carbon tetrachloride proceeds via the reaction: 2 N205 (soln) -----> 4 NO2 (soln) + O2 (soln) The reaction is first order. The rate law for the reaction is rate = a. rate = k [N2O5] b. rate = k [N205]? rate = k [N205]3 с. d. rate = k [NO2] [921

Consider the following chemical equation: Overall Reaction: A B2 + BC - AB + C + B2 The proposed mechanism is as follows: BC – B+ C (slow) A B2 + B = AB+ B2 (fast) What is the rate law? Rate = k[B C] O Rate = k[A B,][B] Rate = k[C] O Rate = k[B][C] Rate k[A B2][B C) Rate = k[A B][B,] Rate = k(A B2]

Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate =(0.0913 s¯¹)[C₁₂05] Suppose a vessel contains Cl₂05 at a concentration of 0.460M. Calculate the concentration of C1₂O5 in the vessel 9.70 seconds later. You may assume no other reaction is important. 25 2 Round your answer to 2 significant digits. [ M x10

3. An experiment was carried out to determine the rate law for the following reaction: 19152 2NO( )+0( ) → 2NO( ) Where the rate law is: par Rate = k[NO] [0] The experiment was repeated three times and the following data recorded: Experiment # Initial [NO] (M) Initial [0] (M) Rate (M/s) 1 ullo2 M0.015 0.015 2 0.030 0.015 3 0.015 0.030 of in Determine the value of x in the rate law (order of reaction with respect to NO) by comparing experiments 1 and 2 in Equation 13 reaction with respect to O₂) by comparing experiments 1 and 3 in equation 13. 0.048 0.192 0.096