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At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k =...

At 3500 K, the following reaction has the rate law Rate = k[H2][Ar], where k = 2.2 x 10^5 M^-1sec^-1

H2(g) + Ar(g) → 2 H(g) + Ar(g)

a. Calculate the rate of reaction when [H2] = 1.0 x 10^-3 M and [Ar] = 7.2x 10^-4 M.

b. Derive an expression for t½ for a second order reaction (Rate = k[A]^2).

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