The rate of iron oxidation by oxygen has the rate law The rate constant k has a

Question

The rate of iron oxidation by oxygen has the rate law
The rate constant k has a value of 9×1013 [s–1 (L/mol)3]. Calculate the observed first order rate constant
When the pH is buffered at pH 6 and the oxygen concentration is kept constant at 2×10–4 M by aeration. The rate of iron oxidation by oxygen has the rate law
The rate constant k has a value of 9×1013 [s–1 (L/mol)3]. Calculate the observed first order rate constant
When the pH is buffered at pH 6 and the oxygen concentration is kept constant at 2×10–4 M by aeration. The rate of iron oxidation by oxygen has the rate law
The rate constant k has a value of 9×1013 [s–1 (L/mol)3]. Calculate the observed first order rate constant
When the pH is buffered at pH 6 and the oxygen concentration is kept constant at 2×10–4 M by aeration.

Explanation / Answer

2Fe(s) + 3/2O2(g) --> Fe2O3(s)

apparant rate Law:

RAte = K*[Fe]^2 * [O2]^1.5

k = 9*10^13

[O2] = 2*10^-4 M

so

RAte = k*[Fe]^2 * [O2]^1.5

rate = (9*10^13)([Fe]^2(2*10^-4)^1.5))

Rate = (2*10^-4)^1.5) * 9*10^13) = 2545*10^8 * [Fe]^2

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