Question

The table shows the concentration of a reactant in the reaction mixture over a period of time.

Answer 1

Option C

The average rate of the reaction over the entire course of the reaction is: $2.0 \times 10^{-3}$

Solution:

Average rate is the ratio of concentration change to the time taken for the change

$Average\ rate = \frac{ \triangle c }{\triangle t }$

The concentration of the reactants changes 1.8 M to 0.6 M

here, the time interval given is 0 to 580 sec

Therefore,

$Average\ rate = \frac{1.8-0.6}{580} \\\\Average\ rate = \frac{1.2}{580} \\\\Average\ rate \approx 2.0 \times 10^{-3}$

Thus option C is correct