For the second-order reaction NO(g)+ O 3 (g)$\to$ NO 2 (g)+ O 2 (g),the rate constant has been measured to be 1.08 $\times$ 10 7 M - 1 s - 1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K - 1 mol - 1 )

The Answer of For the second-order reaction NO(g)+ O 3 (g)$\to$ NO 2 (g)+ O 2 (g),the rate constant has been measured to be 1.08 $\times$ 10 7 M - 1 s - 1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K - 1 mol - 1 )

For the second-order reaction NO(g)+ O 3 (g)$\to$ NO 2 (g)+ O 2 (g),the rate constant has been measured to be 1.08 $\times$ 10 7 M - 1 s - 1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K - 1 mol - 1 )

The Answer of For the second-order reaction NO(g)+ O 3 (g)$\to$ NO 2 (g)+ O 2 (g),the rate constant has been measured to be 1.08 $\times$ 10 7 M - 1 s - 1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K - 1 mol - 1 )

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For the Second-Order Reaction NO(g)+ O₃(g) $\to$ NO₂(g)+ O₂(g),the Rate Constant Has Been Measured to Be 1

Question 104

Multiple Choice

For the second-order reaction NO(g) + O₃(g) $\to$ NO₂(g) + O₂(g) ,the rate constant has been measured to be 1.08 $\times$ 10⁷ M^-¹ s^-¹ at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K^-¹ mol^-¹)

A) $For the second-order reaction NO(g) + O3(g) \to NO2(g) + O2(g) ,the rate constant has been measured to be 1.08 \times 107 M-1 s-1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K-1 mol-1) A) M-1 s-1 B) M-1 s-1 C) M-1 s-1 D) M-1 s-1 E) M-1 s-1$ M^-¹ s^-¹
B) $For the second-order reaction NO(g) + O3(g) \to NO2(g) + O2(g) ,the rate constant has been measured to be 1.08 \times 107 M-1 s-1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K-1 mol-1) A) M-1 s-1 B) M-1 s-1 C) M-1 s-1 D) M-1 s-1 E) M-1 s-1$ M^-¹ s^-¹
C) $For the second-order reaction NO(g) + O3(g) \to NO2(g) + O2(g) ,the rate constant has been measured to be 1.08 \times 107 M-1 s-1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K-1 mol-1) A) M-1 s-1 B) M-1 s-1 C) M-1 s-1 D) M-1 s-1 E) M-1 s-1$ M^-¹ s^-¹
D) $For the second-order reaction NO(g) + O3(g) \to NO2(g) + O2(g) ,the rate constant has been measured to be 1.08 \times 107 M-1 s-1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K-1 mol-1) A) M-1 s-1 B) M-1 s-1 C) M-1 s-1 D) M-1 s-1 E) M-1 s-1$ M^-¹ s^-¹
E) $For the second-order reaction NO(g) + O3(g) \to NO2(g) + O2(g) ,the rate constant has been measured to be 1.08 \times 107 M-1 s-1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K.What is the rate constant at 233 K? (R = 8.3145 J K-1 mol-1) A) M-1 s-1 B) M-1 s-1 C) M-1 s-1 D) M-1 s-1 E) M-1 s-1$ M^-¹ s^-¹

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For the Second-Order Reaction NO(g)+ O3(g) →\to→ NO2(g)+ O2(g),the Rate Constant Has Been Measured to Be 1

For the Second-Order Reaction NO(g)+ O₃(g) $\to$ NO₂(g)+ O₂(g),the Rate Constant Has Been Measured to Be 1