Consider the reaction: -2NO(g) + O2(g) The activation energy for the decomposition of NO2 is 109 kJ/mol. At 653 K, the rate constant was measured to be 1.86 Ms1.At what temperature in Kelvin does the reaction have a rate constant of 4.24 Ms? Type your numeric answer and submit

Consider the reaction : 3A + 2B →  4C Initially, and at some fixed temperature, the reaction proceeds at such a rate that 2.3 millimoles of A are consumed in 1 minute and 12 secondes. The reaction takes place in 1 L. The following table contains the experimental data for the reaction. (Taken from Ball. Physical Chemistry, 2nd edition, 2006) Rate (M/s) [A], M [B], M 1.081 x 10-5 0.660 1.23 6.577 x 10-5 4.01 1.23 6.568 x 10-5 4.01 2.25   c. Determine the partial order on A. Partial order on B is 0. d. What is the order of the reaction.

Consider this reaction: 2NH, (g) → N, (g) +3H, (g) At a certain temperature it obeys this rate law. 2 rate = (0.0581 Ms)[NH,1 Suppose a vessel contains NH, at a concentration of 1.39M. Calculate the concentration of NH, in the vessel 70.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M x10 ?

For the elementary process, CH3Cl(g) + Cl(g)  CH3(g) + Cl2(g), the rate constant increases by a factor of 23.00 when the temperature is raised from 298K to 320K. The value of the gas constant is R = 8.314 J/mol-K. What is the activation energy for this reaction?

a) The reaction of NO2 has been studied as a function of temperature. For the following decomposition reactions, the rate constant is 2.7 × 10-2M-'s-1 at 227 °C and 2.4 x 10-1M-1s-1 at 305 °C. 9. 2 NO2 → 2 N0 + 02 Calculate the activation energy for this reaction. 9. b) Nitrogen oxide converts ozone into molecular oxygen as follows: Оз + NO -> 02 + NO2 The experimental rate law is: Rate = k[03][NO]. Show which of the following mechanism/mechanisms are consistent with the experimental rate law. Mechanism 1: 03 + NO → 02 + NO3 (slow) 0 + 03 → 2 02 (fast) NO3 + NO → 2 NO2 (fast) Mechanism 2: 032 02 + 0 (fast) NO +0 → N02 (slow) Mechanism 3: 03 + NO → 02 + NO2 (slow)

At a certain temperature the rate of this reaction is second order in HI with a rate constant of 0.22M¹s¹: 2 HI(g) → H₂(g) + 1₂ (8) Suppose a vessel contains HI at a concentration of 0.910M. Calculate how long it takes for the concentration of HI to decrease to 0.064 M. You may assume no other reaction is important. Round your answer to 2 significant digits. 0.9 X 圖 图

The thermal decomposition of phosphine (PH3) into phosphorus and molecular hydrogen is a first-order reaction: 4PH₂(g) P4(g) + 6H₂(g) The half-life of the reaction is 31.0 s at 680 °C. Part 1 of 2 Calculate the first-order rate constant for the reaction. Be sure your answer has the correct number of significant digits. 0.0223 s Part: 1 / 2 Part 2 of 2 1 Calculate the time required for 79.0 percent of the phosphine to decompose. Be sure your answer has the correct number of significant digits. x10

Consider the following mechanism for the reduction of nitric oxide: H₂(g) + 2NO(g) → N₂O(g) + H₂O(g) H₂(g) + N₂O(g) → N₂(g) + H₂O(g) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. O yes Ono (1) (2) X 00 e 4

Consider the mechanism. Step 1: 2A — В +С slow Step 2: В +С — Е fast Overall: 2А — Е Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =

The following data were collected for the reaction between hydrogen and nitric oxide at 700°C. 2 H2(g) + 2 NO(g) - 2 H20(g) + N2(g) Experiment [H2]/M [NO]/M Initial rate/M-s-1 0.012 0.031 4.5x10-6 0.0060 0.031 2.2x10-6 3 0.012 0.0155 1.1x10-6 (a) What is the rate law for the reaction? (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad Help Greek - (b) Calculate the rate constant for the reaction. 4.0 (c) Suggest a plausible reaction mechanism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate. Omit states-of-matter from your answer.) First step: chemPad Help Greek - Second step: chemPad Help Greek