Respuesta :
Answer : The correct option is, (A) [tex]2A\rightarrow B+3C[/tex]
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.
As we are given that:
Rate of disappearing component A = [tex]-r_A=4.0\times 10^{-2}M/s[/tex]
Rate of appearing component B = [tex]r_B=2.0\times 10^{-2}M/s[/tex]
Rate of appearing component C = [tex]r_C=6.0\times 10^{-2}M/s[/tex]
The general reaction is:
[tex]aA\rightarrow bB+cC[/tex]
As per question the stoichiometry relation will be:
[tex]\frac{-r_A}{a}=\frac{r_B}{b}=\frac{r_C}{c}[/tex]
Now put the values of rate of following components, we get:
[tex]\frac{4.0\times 10^{-2}}{a}=\frac{2.0\times 10^{-2}}{b}=\frac{6.0\times 10^{-2}}{c}[/tex]
[tex]\frac{4}{a}=\frac{2}{b}=\frac{6}{c}[/tex]
[tex]\frac{2}{a}=\frac{1}{b}=\frac{3}{c}[/tex]
Thus, the stoichiometry relation is:
a : b : c = 2 : 1 : 3
Thus, the required equation will be:
[tex]2A\rightarrow B+3C[/tex]
The stoichiometry for the reaction is given as:
(A) 2 A → B + 3 C
What is 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.
Given:
Rate of disappearing component A = [tex]4.0 * 10^{-2} M/s[/tex]
Rate of appearing component B = [tex]2.0 * 10^{-2} M/s[/tex]
Rate of appearing component C = [tex]6.0 * 10^{-2} M/s[/tex]
From these rates, we can infer that, the stoichiometry relation is:
a : b : c = 2 : 1 : 3
Thus, the required equation will be:
2 A → B + 3 C
So, option A is correct.
Find more information about Rate law here:
brainly.com/question/7694417
