Chemistry final experimental rate constant: K=k'/({H+]^x [I-]^y) = 2.30 1. A proposed mechanism is: H2O2 + H+ + I- --- k1---> HOI + H2O HOI + H+ + I- ---k2---> I2 + H2O Making use of the steady state approximation, derive the rate law. Is the derived mechanism consistent with the experimental rate law? 2. An alternative mechanism has been proposed: H2O2 + I- --- k1/ ---> OI- + H2O OI- + H2O + I- --- k2/ ---> I2 + 2OH Assuming that both mechanisms operate simultaneously, then application of steady state methods gives the following rate law: Rate = k1/ [I-][H2O2] + k1[H+] [I-] [H2O2] = kexptl [H2O2] where kexptl = k1/ [I-] + k1 [H+] [I-] = [I-] { k1/ + k1 [H+] } Do your results suggest this is a more appropriate mechanism? Explain your answer.
Chemistry
final experimental rate constant: K=k'/({H+]^x [I-]^y) = 2.30
1. A proposed mechanism is:
H2O2 + H+ + I- --- k1---> HOI + H2O
HOI + H+ + I- ---k2---> I2 + H2O
Making use of the steady state approximation, derive the rate law.
Is the derived mechanism consistent with the experimental rate law?
2. An alternative mechanism has been proposed:
H2O2 + I- --- k1/ ---> OI- + H2O
OI- + H2O + I- --- k2/ ---> I2 + 2OH
Assuming that both mechanisms operate simultaneously, then application of steady state methods gives the following rate law:
Rate = k1/ [I-][H2O2] + k1[H+] [I-] [H2O2] = kexptl [H2O2]
where kexptl = k1/ [I-] + k1 [H+] [I-] = [I-] { k1/ + k1 [H+] }
Do your results suggest this is a more appropriate mechanism? Explain your answer.
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