Nitric oxide was reacted with chlorine to produce nitrosylchloride according to

Question

Nitric oxide was reacted with chlorine to produce nitrosylchloride according to the following equation: 2NO (g) + CI2(g) -------> 2NOCI (g) The rate constant for this reaction at 25 degrees C is 4.9 x10-6 L/(mol s) while the rate constant at 35 degrees Cis 1.5 x 10-5 L/(mol s). Using this data the energy ofactivation for this reaction is 85 kJ. What is the rate constant at 150 degrees C. using the reactionabove? Nitric oxide was reacted with chlorine to produce nitrosylchloride according to the following equation: 2NO (g) + CI2(g) -------> 2NOCI (g) The rate constant for this reaction at 25 degrees C is 4.9 x10-6 L/(mol s) while the rate constant at 35 degrees Cis 1.5 x 10-5 L/(mol s). Using this data the energy ofactivation for this reaction is 85 kJ. What is the rate constant at 150 degrees C. using the reactionabove?

Explanation / Answer

         According toArrehenius equation ,   ln K1 / K2 = (Ea / R)( 1 /T2 - 1 /T1)                  Ea = 85kJ               T1 = 35oC = 308 K                T2 = 1500C = 423 K                  K1 = 1.5 x 10-5 L /mol s                 K2 = ?                 ln (1.5 x 10-5 / K2) = (85 / 8.314) / ( 1 /423 -1 / 308)            K2 = 1.51 x 10-5 L / mol s          

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