For the non – stoichiometre reaction 2A + B $\to$ C + D, the following kinetic data were obtained in three separate experiments, all at 298 K. .tg {border-collapse:collapse;border-spacing:0;} .tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg th{font-family:Arial, sans-serif;font-size:14px;font-weight:normal;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg .tg-s6z2{text-align:center} .tg .tg-baqh{text-align:center;vertical-align:top} .tg .tg-hgcj{font-weight:bold;text-align:center} Initial Concentration (A) Initial Concentration (B) Initial rate of formation of C (mol L-1 s-1) 0.1 M 0.1 M 1.2 x 10-3 0.1 M 0.2 M 1.2 x 10-3 0.2 M 0.1 M 2.4 x 10-3 The rate law for the formation of C is:

Question

For the non – stoichiometre reaction 2A + B $\to$ C + D, the following kinetic data were obtained in three separate experiments, all at 298 K.

Initial Concentration (A)	Initial Concentration (B)	Initial rate of formation of C (mol L^-1 s^-1)
0.1 M	0.1 M	1.2 x 10^-3
0.1 M	0.2 M	1.2 x 10^-3
0.2 M	0.1 M	2.4 x 10^-3

The rate law for the formation of C is:

${{dc} \over {dt}} = k[A]{[B]^2}$

${{dc} \over {dt}} = k[A]$

${{dc} \over {dt}} = k[A]{[B]}$

${{dc} \over {dt}} = k[A^2]{[B]}$

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