At room temperature, the reaction between NO and O2 to give NO2 is fast while that of between CO and O2 is slow. It is because

Question

At room temperature, the reaction between NO and O2 to give NO2 is fast while that of between CO and O2 is slow. It is because (A) the intrinsic energy of the reaction 2 NO + O2 leftharpoons 2 NO2 is less (B) CO is smaller in size than that of NO (C) CO is poisonous (D) the activation energy for the reaction 2 NO + O2 leftharpoons NO2 is less

Tardigrade Admin · Accepted Answer

Evidently, less is the activation energy, faster is the reaction or greater is the activation energy, slower is the reaction.

Q. At room temperature, the reaction between $NO$ and $O_{2}$ to give $N O_{2}$ is fast while that of between $CO$ and $O_{2}$ is slow. It is because

the intrinsic energy of the reaction $2 NO + O_{2} ⇌ 2 N O_{2}$ is less

$CO$ is smaller in size than that of $NO$

$CO$ is poisonous

the activation energy for the reaction $2 NO + O_{2} ⇌ N O_{2}$ is less

Evidently, less is the activation energy, faster is the reaction or greater is the activation energy, slower is the reaction.

Q. At room temperature, the reaction between NO and O2​ to give NO2​ is fast while that of between CO and O2​ is slow. It is because

the intrinsic energy of the reaction 2NO+O2​⇌2NO2​ is less

CO is smaller in size than that of NO

CO is poisonous

the activation energy for the reaction 2NO+O2​⇌NO2​ is less

Evidently, less is the activation energy, faster is the reaction or greater is the activation energy, slower is the reaction.

Q. At room temperature, the reaction between $NO$ and $O_{2}$ to give $N O_{2}$ is fast while that of between $CO$ and $O_{2}$ is slow. It is because

the intrinsic energy of the reaction $2 NO + O_{2} ⇌ 2 N O_{2}$ is less

$CO$ is smaller in size than that of $NO$

$CO$ is poisonous

the activation energy for the reaction $2 NO + O_{2} ⇌ N O_{2}$ is less