For the following reaction: NO2(g) + CO(g) → NO(g) + CO2(g), the rate law is: Rate = k[NO2]2. If 0.1 mole of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

Question

For the following reaction: NO2(g) + CO(g) → NO(g) + CO2(g), the rate law is: Rate = k[NO2]2. If 0.1 mole of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true? (A) Both k and the reaction rate the reaction rate remain (B) Both k and the reaction rate increase (C) Both k and the reaction rate decrease (D) Only k increases, the reaction rate remain the same

Tardigrade Admin · Accepted Answer

NO 2(g)+ CO (g) longrightarrow NO (g)+ CO 2(g) ∵ Rate of reaction, ((d x/d t))=k[ NO 2]2 ∴ Rate is independent of CO. Hence, on adding more CO to the reaction mixture, both k and rate remain the same.

Q. For the following reaction:
$N O_{2 (g)} + C O_{(g)} \to N O_{(g)} + C O_{2 (g)}$ , the rate law is: Rate = $k [N O_{2}]^{2}$ . If $0.1$ mole of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

Both $k$ and the reaction rate the reaction rate remain

Both $k$ and the reaction rate increase

Both $k$ and the reaction rate decrease

Only $k$ increases, the reaction rate remain the same

Only the reaction rate increases; $k$ remains the same

$N O_{2} (g) + CO (g) ⟶ NO (g) + C O_{2} (g)$

$∵$ Rate of reaction, $(\frac{d x}{d t}) = k [N O_{2}]^{2}$

$∴$ Rate is independent of $CO$ .

Hence, on adding more $CO$ to the reaction mixture, both $k$ and rate remain the same.

Q. For the following reaction: NO2(g)​+CO(g)​→NO(g)​+CO2(g)​, the rate law is: Rate = k[NO2​]2. If 0.1 mole of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?

Both k and the reaction rate the reaction rate remain

Both k and the reaction rate increase

Both k and the reaction rate decrease

Only k increases, the reaction rate remain the same

Only the reaction rate increases; k remains the same

NO2​(g)+CO(g)⟶NO(g)+CO2​(g) ∵ Rate of reaction, (dtdx​)=k[NO2​]2 ∴ Rate is independent of CO. Hence, on adding more CO to the reaction mixture, both k and rate remain the same.