5) NO2(g), (a.k.a. smog! And I don't mean the dragon), reacts with and causes the decay of ozone. Determine the rate law and the value of k for the following reaction using the data provided. NO2(g) +03(g) → NO3(g) + O2(g) [NO2]i (M) [03]i (M) Initial Rate 0.10 0.33 1.42 0.10 0.66 0.25 0.66 2.84 7.10 FULL ANSWER: 6) A data for the reaction in #5 was from experiments performed at room temperature (assume 25 °C). The energy of activation of the reaction is 63 kJ/mole. Use the rate constant you determined above to discover rate constant at -3 °C, which is the temperature of the stratosphere. ANSWER:

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

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The decomposition of nitrosyl bromide is followed                         2 NOBr → 2 NO + Br2   Time (s) [NOBr] (M) 0.00 0.0100 2.00 0.0071 4.00 0.0055 6.00 0.0045 8.00 0.0038 10.00 0.0033    Determine the average rate over the entire experiment.

Given- H2S (g) + O2 (g) → H2O (g) + S8 (g)-Write the expression of the rate in terms of the concentration of eachreactant and product over time.-If the rate of formation of S8 is 0.078 M/s, what is the rate ofdisappearance of H2S?

consider the reaction 2 H2 (g) + O2 (g) = 2H2O (g). Determine the rate in which H2O is formed

Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. 1 rate = (0.471 M¹S -¹) [N₂05]² Suppose a vessel contains N₂O5 at a concentration of 0.800M. Calculate the concentration of N₂O5 in the vessel 8.40 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10

for the reaction between nitrogen monoxide and chlorine to produce nitrosyl chloride 2NO + Cl2 --> 2NOCl it is found that tripling the concentration of both reactants increases the rate by a factor of 27. if only the concentration of chlorine is tripled the rate increases by a factor of 3. give order of this reaction with respect to NO and determine the rate law for the reaction

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A particular reactant decomposes with a half‑life of 117 s117 s when its initial concentration is 0.376 M.0.376 M. The same reactant decomposes with a half‑life of 221 s221 s when its initial concentration is 0.199 M.0.199 M. Determine the reaction order. 2 1 0   What is the value and units of the rate constant for this reaction? ?=k=     Units