The following results were found after completion of Part C in the Experimental procedure: 0.056 M I- and 0.048 M H2O2 were used Run Catalyst Calculated Rate of Reaction (M/s) 1 none 0.031 2 10.00mL of 0.35 M FeCl2 0.52 Assuming the Rate Law = k[I-][H2O2] 2 Calculate the value of k for run 2.  Give your answer to the nearest whole number.

Using a second-order integrated rate law to find concentration change -1 -1 At a certain temperature this reaction follows second-order kinetics with a rate constant of 0.0107 M .S 2NH3 (g) → N2 (g) + 3H2(g) : Suppose a vessel contains NH3 at a concentration of 0.610M. Calculate the concentration of NH3 in the vessel 870. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. Шм ☐ x10 ☑ 00. Ar

Question 30 of 39 Submit The zero order reaction A → Products takes 63.5 minutes for the concentration of A to decrease from 0.970 M to 0.205 M. What is the value of k for this reaction? M/min 1 3 4 C 7 8 9 +/- х 100 Tap here or pull up for additional resources

Consider this initial rate data at a certain temperature in the table for the reaction Determine the rate law. OCI (aq) + (aq)- k= rate = k OH(aq) [OCIT] [OH] →OI (aq) + Cl(aq) [1] [1-1² Answer Bank [OH-]² Trial 1 2 3 4 [OCIT [I lo [OCI ]o (M) (M) 0.00179 0.00179 0.00179 0.00322 0.00281 0.00179 0.00179 0.00322 Determine the value of the rate constant for this reaction and the correct units. Units [OH Jo (M) 0.490 0.490 0.681 0.867 Initial rates (M/s) 0.000440 0.000792 0.000497 0.000448

1 ok S t nces Experiment [H₂] [NO] 0.010 0.025 Be sure to answer all parts. The following data were collected for the reaction between hydrogen and nitric oxide at 700°C: 2H₂(g) + 2NO(g) > 2H₂O(g) + N₂(g) 1 2 3 Initial rate (M/s) 2.4 x 10-6 1.2 × 10-6 0.010 0.0125 0.6 x 10-6 0.0050 0.025 5 attempts left (b) Calculate the rate constant. Check my work (a) Determine the order of the reaction. Enter a number in the field below. Number: Units: