Question

For the net reaction: 2AB + 2C → A2 + 2BC, the following slow first steps have been proposed. 2C + AB → AC + BC 2AB → A2 + 2B C + AB → BC + A AB → A + B What rate law is predicted by each of these steps? C

Answer 1

Answer : The rate law expression for the following reactions are:

(1) $\text{Rate}=k[C]^2[AB]$

(2) $\text{Rate}=k[AB]^2$

(3) $\text{Rate}=k[C][AB]$

(4) $\text{Rate}=k[AB]$

Explanation :

Rate law : It is defined as the expression which expresses the rate of the reaction in terms of molar concentration of the reactants with each term raised to the power their stoichiometric coefficient of that reactant in the balanced chemical equation.

The general reaction is:

$A+B\rightarrow C+D$

The general rate law expression for the reaction is:

$\text{Rate}=k[A]^a[B]^b$

where,

a = order with respect to A

b = order with respect to B

R = rate  law

k = rate constant

[A] and [B] = concentration of A and B reactant

Now we have to determine the rate law for the given reaction.

(1) The balanced equations will be:

$2C+AB\rightarrow AC+BC$

In this reaction, C and AB are the reactants.

The rate law expression for the reaction is:

$\text{Rate}=k[C]^2[AB]$

(2) The balanced equations will be:

$2AB\rightarrow A_2+2B$

In this reaction, AB is the reactant.

The rate law expression for the reaction is:

$\text{Rate}=k[AB]^2$

(3) The balanced equations will be:

$C+AB\rightarrow BC+A$

In this reaction, C and AB are the reactants.

The rate law expression for the reaction is:

$\text{Rate}=k[C][AB]$

(4) The balanced equations will be:

$AB\rightarrow A+B$

In this reaction, AB is the reactant.

The rate law expression for the reaction is:

$\text{Rate}=k[AB]$

Answer 2

The rate law that is predicted by each of these steps include:

1. $R_o = k[C]^2[AB]$

2. $R_o = k[AB]$

3. $R_o = k[C][AB]$

4. $R_o = k[AB]$

Given the following net reaction:

• $2AB + 2C \rightarrow A_2 + 2BC$

Rate law is also referred to as a rate reaction and it can be defined as an expression that relates the initial or forward rate of a chemical reaction with the concentrations or partial pressures of the chemical reactants and their constant parameters.

Mathematically, rate law is given by the formula:

$R_o = k[A]^x[B]^y$

Where:

• k is the rate constant.

• $R_o$ is the rate of a chemical reaction.

• A is the concentration of reactant A.

• B is the concentration of reactant B.

• x is the order of reaction with respect to reactant A.

• y is the order of reaction with respect to reactant B.

Next, we would write rate law for each steps of the net reaction.

Step 1:

$2C + AB \rightarrow AC + BC$

$R_o = k[C]^2[AB]$

Step 2:

$2AB \rightarrow A_2 + 2B$

Note: This is a first-order reaction.

$R_o = k[AB]$

Step 3:

$C + AB \rightarrow BC + A$

$R_o = k[C][AB]$

Step 4:

$AB \rightarrow A + B$

Note: This is a first-order reaction.

$R_o = k[AB]$

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