Click in the answer box to activate the palette. Derive the rate law for the decomposition of ozone (in terms of k1, k2, and k_1) from the following steps. Ozone, O3, decomposes to molecular oxygen, O2, via the following process: 203(g) → 302g) The rate law for the decomposition of ozone to molecular oxygen is rate = [02] The mechanism proposed for this process is 03 0+ 02 0+03 → 202 What is the rate law in terms of k1, k2, and k_1? rate =

A chemistry graduate student is studying the rate of this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) She fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time [C1,05] (seconds) 0 0.400M 10. 0.263 M 20. 0.173 M 30. 0.114M 40. 0.0751M Use this data to answer the following questions. Write the rate law for this reaction. x10 Calculate the value of the rate constant k. X Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 Ś ?

: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9

Consider this reaction: 2SO3 (g) →2SO₂(g) + O₂(g) At a certain temperature it obeys this rate law. rate = (0.894 M¹-s¹) [S0₂] Suppose a vessel contains SO3 at a concentration of 0.390 M. Calculate the concentration of SO3 in the vessel 8.60 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M Explanation Check 0 10 Q Search a Ⓒ2023 McGraw Hill LLC. All Rights Reserved. Terms of Use O Privacy Center

13.102 Chlorine oxide (CIO), which plays an important role in the depletion of ozone (see Problem 13.101), decays rapidly at room temperature according to the equation 2C10(g) Cl₂(g) + O₂(g) From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) 0.12 x 10-³ 0.96 x 10-³ 2.24 x 10-³ 3.20 x 10-³ 4.00 x 10-³ [CIO] (M) 8.49 x 10-6 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6

Consider this reaction: 2H1 (g) → H₂(g) +1₂(e) At a certain temperature it obeys this rate law. rate = (0.345-¹) [HI] Suppose a vessel contains HI at a concentration of 0.730M. Calculate how long it takes for the concentration of HI to decrease by 86.0%. You may assume no other reaction is important. Round your answer to 2 significant digits. 0. 08

Consider the reaction for the formation of ammonia, NH3:                              N2(g) + 3 H2(g) --> 2 NH3(g) Which is the correct rate expression for this reaction?

23. Consider the following reaction: 2 NO2(g) + O3(g)  N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)]     Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____  M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____  M/s

Consider this reaction: 2SO3 (g) →2SO₂ (g) + 0₂ (8) At a certain temperature it obeys this rate law. rate= (0.00626 s¹)[03] Suppose a vessel contains SO3 at a concentration of 0.250M. Calculate the concentration of SO3 in the vessel 99.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 X Ś