The data in the table concern the lactonization of hydroxyvaleric acid at 25 degrees Celsius. They give the concentration $C(t)$ of this acid in moles per liter after $t$ minutes.
$$\begin{array}{|c|c|} \hline t & C(t) \\ \hline 0 & .0800 \\ 2 & .0570 \\ 4 & .0408 \\ 6 & .0295 \\ 8 & .0210 \\ \hline \end{array}$$
Find the average rate of reaction for the following time intervals:

(a) $2 \leq t \leq 6$, (b) $2 \leq t \leq 4$, (c) $0 \leq t \leq 2$

(By plotting a graph, can you see why the instantaneous rate of change is approximately -.01 (moles/L)/min?)

(a) (moles/L)/min
(b) (moles/L)/min
(c) (moles/L)/min