Nitrogen dioxide gas decomposes at high temperature according to this reaction:   2NO2(g) ⟶2 NO(g)  + O2(g) The following data were collected at 200°C.  Determine the value of the rate constant.  (Hint: determine the rate law first, then use one of the experiments to determine the value of k)  Enter a number to 2 decimal

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

5

3. Consider the reaction below: 2NO (g) + Cl,(g)'n 2NOCI (g) A mechanism involving these steps has been proposed for the reaction: Step 1: NO (g) + Cl,(g)'n NOCI, (g) Step 2: NOCI, (g) + NO(g)'n 2NOCI (g) The rate law for the reaction is given by rate = k[NO][Cl]. (a) What is the reaction intermediate? (b) Which is the rate-determining step? (c) Is the rate-determining step unimolecular, bimolecular, or termolecular? Why?

Please answer this question within 5 minutes, i will rate you for sure.

Consider this reaction: 2NH, (g) - N2 (g) +3H, (g) At a certain temperature it obeys this rate law. rate =(0.0103 s")[NH,] S Suppose a vessel contains NH, at a concentration of 0.170M. Calculate the concentration of NH, in the vessel 68.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10

The data shows that the rate depends on the concentration of the reactants. How else can a chemist increase the rate of reaction?

Consider this reaction: CICH, CH, CI (g) → CH,CHCI (g) +HC1 (g) At a certain temperature it obeys this rate law. rate = (0.0361 s")[CICH,CH,CI] Suppose a vessel contains CICH,CH,Cl at a concentration of 0.860M. Calculate the concentration of CICH,CH,Cl in the vessel 36.0 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (8.98 × 10-4 ')[c,os] -1 S Suppose a vessel contains Cl₂05 at a concentration of 1.40M. Calculate the concentration of Cl₂O5 in the vessel 690. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.

Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0017 M.s¹: Suppose a 300. mL flask is charged under these conditions with 450. mmol of hydrogen iodide. How much is left 200. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 2 HI (9) H2(g)+1₂(g) B = X x10