T Determine the rate law and the value of k for the following reaction using the

Question

T Determine the rate law and the value of k for the following reaction using the data provided. CO(g) + CI_2(g) rightarrow COCI_2(g) [CO]_i(M) 0.25 0.25 0.50 [CI_2]_i(M) 0.40 0.80 0.8 Initial Rate (M^-1 s^-1) 0.696 1/97 3.94 Rate = 11 M^-3/2_s^-1[CO][CI_2]^3/2 Rate = 36 M^-1.8_s^-1 [CO][CI_2]^2.8 Rate = 17 M-2_s^-1 [CO][CI_2]^2 Rate = 4.4 M^-1/2_s^1 [CO][CI_2]^1/2 Rate = 18 M^-3/2s^-1 [CO]^2[CI_2]^1/2 which of the following represents the integrated rate law for a first-order reaction? In [A]_t/[A]_0 = -kt 1/[A]_t-1/[A]_0=kt [A]_t-[A]_0 = -kt k= Ae (-Ea/RT) In k2/k1=E_a/R[1/T] + In A

Explanation / Answer

8. rate of the reaction is affected by both reactant therefore the reaction follow second order reaction therefore the answer is option C

9.

integrate rate law of first order reaction

ln[A] = -kt +ln[Ao] = -kt = ln[A]t/[Ao]

answer is option A

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