Determine the missing initial rate for the following $\frac{3}{2}$ order reaction given the following information: $$\begin{array} { l | l }
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \
\hline 0.0174 & 0.16 \
0.0361 & ? \
0.0996 & 2.2
\end{array}$$

Question

Determine the missing initial rate for the following $\frac{3}{2}$ order reaction given the following information: $$\begin{array} { l | l } 
{ [ \mathrm { A } ] \left( \mathrm { mol } \mathrm { L } ^ { - 1 } \right) } & \text { Initial Rate } \left( \mathrm { mol } \mathrm { L } ^{- 1} \mathrm {~s} ^ { - 1 } \right) \
\hline 0.0174 & 0.16 \
0.0361 & ? \
0.0996 & 2.2
\end{array}$$

Quizplus · Accepted Answer

The rate law for a $\frac{3}{2}$ order reaction is:$$Rate = k[A]^{\frac{3}{2}}$$We can use the given data to find the value of the rate constant (k):$$\frac{0.16}{0.0174^{\frac{3}{2}}} = k = 1.43 \mathrm{~mol}^{-1/2} \mathrm{~L}^{1/2} \mathrm{~s}^{-1}$$Now we can use the rate law to calculate the missing initial rate:$$Rate = 1.43 \mathrm{~mol}^{-1/2} \mathrm{~L}^{1/2} \mathrm{~s}^{-1} \times (0.0361 \mathrm{~mol} \mathrm{~L}^{-1})^{\frac{3}{2}} = 0.38 \mathrm{~mol} \mathrm{~L}^{-1} \mathrm{~s}^{-1}$$

Determine the Missing Initial Rate for the Following 32\frac{3}{2}23​ Order Reaction Given the Following Information

Determine the Missing Initial Rate for the Following $\frac{3}{2}$ Order Reaction Given the Following Information