1. A certain reaction has an activation energy of 54.0 kJ/mol. As the temperatur
ID: 851755 • Letter: 1
Question
1. A certain reaction has an activation energy of 54.0 kJ/mol. As the temperature is increased fromm 22 degree C to a higher temperature, the rate constant increases by a factor of 7.00. Calculate the higher temperature. (SHOW WORK!)
2. Draw the energy profile for an exothermic reaction. Label on the diagram the reactants and products, the activation energy for the forward reaction, and label the energy change for the reaction. Be sure to label the axes. Repeat the process for an endothermic reaction.
Exothermic Endothermic
Explanation / Answer
We Know that:
According to Arrhenius equation:
log(K2/K1) = Ea/ 2.303 R ( 1/T1- 1/T2)
The given data:
K1 = K
K2 = 7K
Ea = 54 kJ/mol
T1 = 220C = 298 K
T2 = ? K
Substituting the values in the above Arrhenius equation we get:
log 7K / K = 54 kJ/mol / 2.303 x 8.314x 10-3 kJ /mol-K ( 1/ 298 - 1/T2)
1/T2 = 0.0030
T2 = 327.22 K
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