Rate constants and determination of activation energy. Initial concentrations: 1

Question

Rate constants and determination of activation energy. Initial concentrations: 1.6M acetone 0.4M HCl 0.001M I2 Reaction times at each temp and rate of reaction; 283degres K..... 383 seconds.... 2.70x10^-6 294 degrees K.... 110 seconds... 9.09x10^-6 303 degrees K..... 35 seconds.... 2.86x10^-5 What is the reaction rate constant at each temp? (k=rate/([Ac]o^m[I2]o^n[H+]o^p) and assume m=1, n=0, and p=1 Use the equations (1/T)(K^-1) and k(L/mol-s) and ln(k) for each temperature i am not sure how to use these equations

Explanation / Answer

Activation energy is the amount of energy required to initiate a chemical reaction. The activation energy can be determined from reaction rate constants at different temperatures by the equation

ln(k2/k1) = Ea/R x (1/T1- 1/T2)

where
Eais the activation energy of the reaction in J/mol
R is the ideal gas constant = 8.3145 J/K

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