Second Order Reaction Kinetics

Question

The removal of phosphate, [P], during water treatment is a second-order reaction with the rate law $-\frac{d[P]}{dt}=k[P]^2$ . The rate constant is $k=0.2$ L/(mg·min). The table below summarizes the relationship for this reaction.

Time (min)	1/[P] (L/mg)
0	1/[P₀]
t	k*t + 1/[P₀]

All of the following statements about this reaction are true EXCEPT:

| Time (min) | 1/[P] (L/mg) |
|------------|---------------|
| 0          | 1/[P₀]        |
| t          | k*t + 1/[P₀]  |

All of the following statements about this reaction are true EXCEPT:

Accepted Answer

A plot of $$1/[P]$$ versus time yields a straight line with a slope equal to $$-0.2$$.

Answer

The reaction is second-order with respect to phosphate.

Answer

Integration of the rate law gives $$1/[P]=k*t+1/[P₀]$$, where $[P₀]$ is the initial phosphate concentration.

Answer

The half-life for a second-order reaction depends on the initial phosphate concentration.

Second Order Reaction Kinetics

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