Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l }
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \
\hline 0.35 & 0.038 \
0.70 & 0.038 \
1.05 & 0.038
\end{array}$$

Question

Without performing complex calculations,determine the order of a reaction that has the following initial rates for the specified starting concentration: $$\begin{array} { l | l } 
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \
\hline 0.35 & 0.038 \
0.70 & 0.038 \
1.05 & 0.038
\end{array}$$

Quizplus · Accepted Answer

Since the initial rate is constant, the reaction order with respect to [A] is zero. This can be seen from the fact that doubling [A] does not result in a doubled rate, indicating that there is no dependence of the rate on [A].

Without Performing Complex Calculations,determine the Order of a Reaction That