Nitrogen monoxide, NO, reacts with hydrogen, H₂, according to the following equation.

What would the rate law be if the mechanism for this reaction were as follows?
(Rate expressions take the general form: rate = k . [A]a . [B]b.)
(slow)
(fast)

Answer : The rate law for the overall reaction is,

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 the mechanism for the reaction :

Step 1 :    (slow)

Step 2 :     (fast)

Overall reaction :

The rate law expression for overall reaction should be in terms of .

As we know that the slow step is the rate determining step. So,

The slow step reaction is,

The expression of rate law for this reaction will be,

Hence, the rate law for the overall reaction is,

the electronic configuration of an atom with eight electrons is 1s²2s²2p⁴. the orbital diagrams are shown in the figure.

as per the hunds rule:

1. electrons tend to avoid being in the same orbital as per as practicable.

2. electrons in different orbitals of the same energy will have their spin parallel.

this can be illustrated from the multiplicity of the orbitals of the atom. as there are four electrons in the p orbital and p orbital has 3 sub-shells. the electrons can be fed in different ways as shown in the figure but the correct orbital diagram will be as per the hunds rule.

yes

ya te ayud espera