Question

The data for the reaction is A + B $\to$ C is
$\begin{array}{cccc}Exp.& [A{]}_0& [B{]}_0& Initialrate\\ 1& 0.012& 0.035& 0.10\\ 2& 0.024& 0.035& 0.80\\ 3& 0.012& 0.070& 0.10\\ 4& 0.024& 0.070& 0.80\end{array}$

• A. $r=k[B{]}^3$
• B. $r=k[A{]}^3$
• C. $r=k\left[A\right][B{]}^4$
• D. $r=k\left[A{]}^2\right[B{]}^2$

Answer 1

The correct option is B $r=k[A{]}^3$

A quick way to solve this would be to look at rows one and two. Straight away you can tell that rate does not depend on [B]