Question

At room temperature, the reaction between $NO$ and $O_2$ to give $N{O}_2$ is fast, while that between $CO$ and $O_2$ is slow. It is due to:

• A. CO is smaller in size than that of NO
• B. CO is poisonous
• C. the activation energy for the reaction, $2NO+O_2\to 2N{O}_2$ is less than $2CO+O_2\to 2C{O}_2$
• D. none of the above

Answer 1

The correct option is C the activation energy for the reaction, $2NO+O_2\to 2N{O}_2$ is less than $2CO+O_2\to 2C{O}_2$

At room temperature, the reaction between $NO$ and $O_2$ to give $N{O}_2$ is fast, while that between $CO$ and $O_2$ is slow. It is due to the activation energy for the reaction, $2NO+O_2\to 2N{O}_2$ is less than $2CO+O_2\to 2C{O}_2$.

Reactions having lower energy of activation occurs more fast under similar experimental conditions.