chemistry

The breakdown of p-nitrophenylphosphate at pH 2.6 is a first order hydrolysis process..
a) 12.5mmol of NPP were dissolved in 200mL of water at 77degrees celcius after 50mins the amount of NPP dropped to 10mmol. Calculate the average rate of this reaction and the rate constant for this process.
B) using the arrhenius equation (given A=6 10^11 s^-1) compute the activation energy of this reaction.

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asked by N
  1. avg rate = (12.5-10)/50 min = ? mM/min.

    rate = k(NPP). You know NPP initially and the rate, solve for k.

    Plug all of this into the Arrhenius equation an solve for activation energy.

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  2. for the part rate= k(NPP) what are the units of measurements at the end ?

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    posted by deirdre

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