What are the units of k in the following rate law if the rate of the reaction is M/s? s stands for seconds Rate = k[X]°[Y]° %3D O SM²² (or s/M²) O M/s (or Msec-l) O M's! O 1/s (or sec*1) O Ms

O KINETICS AND EQUILIBRIUM = 3/5 Using first- and second-order integrated rate laws Consider this reaction: 2N₂O5 (g) → 2N₂O4 (g) + O₂(g) At a certain temperature it obeys this rate law. rate = (1.3 M¹-s¯¹) [₂0₁] olo Suppose a vessel contains N₂O5 at a concentration of 1.20M. Calculate the concentration of N₂O5 in the vessel 7.30 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. M X Explanation Check Chelsea V @ EH

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6. The oxidation of Br¯ by Br03 in acidic solution (H*) is described by the equation 5 Br (aq) + Br03 (aq) + 6 H* (aq) З Вrz (aq) + 3 H,0() Initial [Br ] (M) Initial [BrO3] (M) Initial [H*] (M) Initial Reaction Rate (M/s) 4.2 x 10-3 8.4 x 10-3 1.055 x 10-3 4.2 x 10-3 Experiment 1 0.404 0.250 0.100 2 0.808 0.250 0.100 3 0.404 0.125 0.250 0.100 4 0.404 0.050 (a) What is the reaction order with respect to each reactant? (b) Write the rate law. (e) What are the units of the rate constant (k)? [Hint: The units of the rate constant should match the overall reaction order

for this reaction (including orders). Also give the overall order for this reaction: rate law: overall order = %3D 3. Calculate the rate constant, k, for this reaction (use the data from Experiment #1, show all your work): wollood 4. Explain exactly what experiment(s) must be performed in order to

Determine order of reaction with aspect To A show reasoning determine order of reaction with respect to B showing reason write rate of reaction what are units of rate constant with reasoning  Determine value of K

What is the rate law for this reaction? Br Na CH;S S SCH3 DMSO ORate = k [C6H11 ] CH, Br ORate k [C6H11 CH2 SCH3] [CH3 S] ORate k [CH3 S ] O Rate k [C6H11 ] [CH3 S] CH, Br

Q6