$$k = 0.25\ \text{M}^{-1}\text{s}^{-1}$$

Question 1

The plot above shows $$\frac{1}{[A]_0}$$ versus time for a reaction. What is the order of the reaction with respect to A?

Accepted Answer

Second order

Question 2

Given the plot above, which integrated rate law equation best describes the reaction?

Accepted Answer

$$\frac{1}{[A]_t} = \frac{1}{[A]_0} + kt$$

Question 3

If the slope of the plot above is 0.25 $$	ext{M}^{-1}	ext{s}^{-1}$$, what is the rate constant $$k$$ for the reaction?

Accepted Answer

$$k = 0.25\ 	ext{M}^{-1}	ext{s}^{-1}$$

Question 4

For a reaction with the plot shown above, what happens to the half-life as the initial concentration of A increases?

Accepted Answer

The half-life decreases

Question 5

Which of the following statements is true for the reaction depicted in the plot above?

Accepted Answer

The rate of reaction is proportional to $$[A]^2$$

Determining Reaction Order from a Concentration vs. Time Plot

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