Answer:
a. r = k. [A]¹. [B]².[C]⁰
b. 3
c. 2
d. 4
e. 1
f. 8
Explanation:
A reaction in which A, B, and C react to form products is first order in A, second order in B, and zero order in C.
a. Write a rate law for the reaction.
r = k. [A]¹. [B]².[C]⁰
where,
r is the <em>rate of the reaction</em>
k is the <em>rate constant</em>
[X]ⁿ are the <em>molar concentrations</em> of each reactant raised to its <em>reaction order</em>
b. What is the overall order of the reaction?
The overall order of reaction is the sum of the individual orders of reaction, that is, 1 + 2 + 0 = 3.
c. By what factor does the reaction rate change if [A] is doubled (and the other reactant concentrations are held constant)?
If A is doubled, then:
r' = k. [2A]¹. [B]².[C]⁰= 2 k. [A]¹. [B]².[C]⁰ = 2 . r
The factor is 2.
d. By what factor does the reaction rate change if [B] is doubled (and the other reactant concentrations are held constant)?
If B is doubled, then:
r' = k. [A]¹. [2B]².[C]⁰ = 4. k. [A]¹. [B]².[C]⁰ = 4 . r
The factor is 4.
e. By what factor does the reaction rate change if [C] is doubled (and the other reactant concentrations are held constant)?
If C is doubled, then:
r' = k. [A]¹. [B]².[2C]⁰ = 1. k. [A]¹. [B]².[C]⁰ = 1 . r
The factor is 1.
f. By what factor does the reaction rate change if the concentrations of all three reactants are doubled?
r' = k. [2A]¹. [2B]².[2C]⁰ = 2.4.1.k. [A]¹. [B]².[C]⁰ = 8 .r
The factor is 8.
