Question

justify the statement in rate law . components x and y may or may not be equal to stoichiometric coefficients​

Answer 1

AnswEr :

$\underline{\underline{\sf Rate \ Law \colon}}$

Rate Law of an equation is an expression that shows the dependence of the rate of reaction on the concentration of the active masses.

Assume a reaction $\sf aA + bB \longrightarrow cC + dD$

Rate Law would be :

$\sf r \propto [A]^a [B]^b$

On the basis of steps in a reaction,there are classified into :

• Elementary Reaction : One step reactions

• Complex Reactions : Multiple step reactions

If the given reaction is elementary,

• $\sf r = k [A]^a [B]^b$

Here,

The variables are equal to the stoichiometric coefficients

If the given reaction is complex,

• $\sf r = k[A]^x[B]^y$

Here,

The variables may or may not be equal to the stoichiometric coefficients

Since there are multiple steps in complex reactions,the concentration of the reacting species is variable. As a result,the rate of the reaction is determined by slowest step termed as Rate Determining Step