Explain what is the constant k for the reaction

Reference no: EM13253570

4A + 2B + C --> D + 2E

a) Write the rate expression for this reaction. What is the rate appearance of D if the rate of dissappearance of A is 4.80x10^-6 M/sec?

b) using collision theory, explain why this reaction does not occur in one step.

c) derive the rate law for this reaction

[A] .300 .600 .300 .300
[B] .0303 .0303 .0909 .0303
[C] .100 .100 .100 .200
Rate (M/s) 4.8E-6 1.92E-5 1.44E-5 9.60E-6

d) what is the overall order of this reaction?

e) what is the constant k for this reaction?

f) what is the rate of the reaction if the initial concentrations of [A] = .400M, [B]= .0500M and [C]= .075M?

Reference no: EM13253570

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