The reaction A + 2B + C → Products has a rate law of Rate = k[A]²[B]. By what factor would the reaction rate change if [A] is tripled?

Answer 1

The rate law for the reaction A + 2B + C → Products is given as Rate = k[A]²[B], where [A], [B], and [C] represent the concentrations of the reactants A, B, and C, respectively, and k is the rate constant.

To determine how the reaction rate changes when [A] is tripled, we can use the following relationship between the rate and concentration:

Rate = k[A]²[B]

If [A] is tripled, then its concentration becomes 3[A]. Substituting this into the rate law, we get:

Rate' = k(3[A])²[B] = 9k[A]²[B]

where Rate' is the new rate of the reaction.

To find the factor by which the reaction rate changes, we can divide the new rate by the original rate:

Rate' / Rate = (9k[A]²[B]) / (k[A]²[B]) = 9

Therefore, if [A] is tripled, the reaction rate will increase by a factor of 9.