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At room temperature, the reaction between \( \mathrm{NO} \) and \( \mathrm{O}_{2} \) to give \( \mathrm{NO}_{2} \) is fast, while that between \( \mathrm{CO} \) and \( \mathrm{O}_{2} \) is slow. It is due to:
(A) \( \mathrm{CO} \) is smaller in size than that of \( \mathrm{NO} \)
(B) \( \mathrm{CO} \) is poisonous
(C) the activation energy for the reaction, \( 2 \mathrm{NO}+\mathrm{O}_{2} \rightarrow 2 \mathrm{NO}_{2} \) is less than \( 2 \mathrm{CO}+\mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2} \)
(D) none of the above
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