  DarianaDeducing a rate law from the change in concentration over timeA chemistry graduate student is studying the rate of this reaction:H2CO, (ag) H20 (ag)+Co, (ag)She fills a reaction vessel with HCO2 and measures its concentration as the reaction proceeds:H,Co3]timeminutes)00.800 M10.0.377 M20.0.246 M300.183 M40.0.146 MUse this data to answer the following questions.rate kWrite the rate law for this reaction.Calculate the value of the rate constant k.?XRound your answer to 2 significant digits. Also besure your answer has the correct unit symbol. DarianaUsing an integrated rate law for a first-order reactionConsider this reaction2HI (g)H (g)+I, (e)At a certain temperature it obeys this rate law.rate (0.00981 s[HI]Suppose a vessel contains HI at a concentration of 0.460 M. Calculate the concentration of HI in the vessel 65.0 seconds later. You may assume no otherreaction is important.Round your answer to 2 significant digits?X

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The rate law of a reaction is expressed as: help_outlineImage TranscriptioncloseA B >C+ D Rate k [A] [BJb Where, k rate constant [A], [B concentration of reactants a+b order of the reaction fullscreen
Step 3

Now, we need to find the order of the reaction. This can be done by plotting graphs of time versus concentration. If the time vs [conc] graph gives a straight line, it will be a zero order re... help_outlineImage TranscriptioncloseIn [H2CO3 Time [H2CO3] 1/H2CO3] 0 0.800 -0.223 1.25 0.377 2.652 10 -0.976 20 0.246 -1.402 4.065 30 5.464 0.183 -1.698 40 0.146 -1.924 6.849 time vs [conc] time vs In [conc] time vs 1/[conc] .NK. 50 0.5 0 20 40 60 0 20 40 60 Time Time Time fullscreen

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Chemical Kinetics 