Determine the rate law and rate constant for the following reaction. Don't forget the units. Some of the numbers are blurry. (The concentrations for H* are x 10-5 and the rates are x 10-7 with the last value being x10-8) 10, (aq) + 81(aq) + 6H*(aq) → 31, (aq) + 2 H₂O(aq) Trial [103] Initial Rate (M/s) 1 0.0050 2.70 x 10 2 0.0100 5.40 x 10 3 0.0050 6.07 x 10 4 0.0050 6.75 x 10 0.030 0.030 0.045 0.030 [H] 2.0 x 10 2.0 x 10 2.0 x 10 1.0 x 10

Chlorine dioxide reacts in basic water to form chlorite and chlorate according to the following chemical equation: 2C1O₂(aq) + 2OH(aq) → CIO₂ (aq) + CIO3(aq) + H₂O(1) Under a certain set of conditions, the initial rate of disappearance of chlorine dioxide was determined to be 2.30 x 10-1 M/s. What is the initial rate of appearance of chlorite ion under those same conditions? O 5.75 x 10-2 M/s O 1.15 x 10-¹ M/s O 2.30 x 10-1 M/s O 4.60 x 10-¹ M/s O 9.20 x 10-1 M/s

If Δ[Br2]ΔtΔ[Br2]Δ� = 4.7×10−6 M/sM/s , what is the value of Δ[ClO−2]ΔtΔ[ClO2−]Δ� during the same time interval? Express your answer to two significant figures and include the appropriate units. What is the average rate of consumption of Br−Br− during the same time interval? Express your answer to two significant figures and include the appropriate units.

-1 -1 At a certain temperature the rate of this reaction is second order in NH¸OH with a rate constant of 1.99M 4 NH,OH (aq) → NH; (aq)+ H,O (aq) Suppose a vessel contains NH,OH at a concentration of 1.46M. Calculate the concentration of NH,OH in the vessel 1.80 seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits. OM x10

I am taking an online chem class and it’s harder than I thought. I have the answers to my whole study guide but I want to understand the WHY of the answers. Thank you!

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A value of k is found from the rate equation Rate = k[A]M[B]". If m-4 and n-2 and the unit for the initial rate is M/h. The unit of k is found to be M* h1 (M to the power of x h to the power of minus 1). What is the value of x?

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Sort the following elementary reactions as unimolecular (1), bimolecular (2) or termolecular (3) and write down the rate law expression for that step Elementary step from reaction mechanism Molecularity Rate law for elementary step (CH3)3CBR → (CH3);C* + Br 2NO2 → N204 CH;CI +I → CH3I + Cl H* + Br - + H202 → HOB + H20 ONBR + ONBr → NO + NO + Brz N2O2 → NO + NO 03 > 02 + 0

Be sure to answer all parts. The reaction between NO2 and CO to produce NO and CO2 is thought to occur in two steps: Step 1: NO2 + NO2     NO + NO3 Step 2: NO3 + CO     NO2 + CO2 The experimental rate law is rate = k[NO2]2. (a) Write the equation for the overall reaction. Do not include phase abbreviations.      (b) Identify the intermediate(s).     NO3    NO2    NO    CO2    CO (c) Identify the rate-determining step.     Step 1    Step 2    Neither step