For the reaction 2A + B $ \to $ C, the values of initial rate at diffrent reactant concentrations are given in the table below. The rate law for the reaction is : .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} [A] (mol L-1) [B] (mol L-1) Initial Rate (mol L-1s-1) 0.05 0.05 0.045 0.10 0.05 0.090 0.20 0.10 0.72

Question

For the reaction 2A + B $ \to $ C, the values of initial rate at diffrent reactant concentrations are given in the table below. The rate law for the reaction is :

[A] (mol L^-1)	[B] (mol L^-1)	Initial Rate (mol L^-1s^-1)
0.05	0.05	0.045
0.10	0.05	0.090
0.20	0.10	0.72

Rate = k[A][B]²

Rate = k[A]²[B]²

Rate = k[A]²[B]

Rate = k[A][B]

Solution

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