• # question_answer For the reaction $2A+B\to C,$ the values of initial at different reactant concentrations are given in table below. The rate law for the reaction is: [A] $(mol\,{{L}^{-\,1}})$ [B] $(mol\,{{L}^{-\,1}})$ Initial Rate $(mol\,L{{\,}^{-\,1}}s{{\,}^{-1}})$ 0.05 0.05 0.045 0.10 0.05 0.090 0.20 0.10 0.75 A)         Rate = $k[A][B]$           B) Rate = $k[A]{{[B]}^{2}}$ C)        Rate = $k{{[A]}^{2}}{{[B]}^{2}}$    D) Rate =$k{{[A]}^{2}}[B]$

 $r=k{{[A]}^{\rho }}{{[B]}^{q}}$ $\frac{{{r}^{2}}}{{{r}_{1}}}={{\left[ \frac{{{A}_{2}}}{{{A}_{1}}} \right]}^{\rho }}{{\left[ \frac{{{B}_{_{2}}}}{{{B}_{1}}} \right]}^{q}}$ ${{2}^{I}}={{2}^{\rho }}$               $(p=1)$ $\frac{{{r}^{3}}}{{{r}_{2}}}={{\left[ \frac{{{A}_{3}}}{{{A}_{2}}} \right]}^{I}}{{\left[ \frac{{{B}_{3}}}{{{B}_{2}}} \right]}^{q}}$ $\frac{0.720}{0.090}=2{{(2)}^{q}}$ $\frac{720}{90\times 2}={{2}^{q}}=4={{2}^{2}}$ $q=2$ $r=k{{(A)}^{I}}{{[B]}^{2}}.$