Question

If a reactant has a -1 order, what happens to the initial rate when the concentration of that reactant increases by a factor of two?

Answer 1

Answer:

$\dfrac{1}{2}$

Explanation:

Let assume that X and Y are the reactants of a given reaction.

Then the rate can be expressed as:

rate = k[X][Y]

Suppose the concentration of X is quadrupled and the rate is doubled.

Then. we have;

$2 \times rate = k[4X]^{\dfrac{1}{2}} [Y]$

So, the initial rate of the concentration will be $\dfrac{1}{2}$ when the concentration of the reactant is increased by a factor of two.