Answer 7.
Expression for rate constant of given reaction (Arrhenius equation) can be written as follows:
Where, k = Rate constant
A = Arrhenius factor
Ea = activation energy = 274 kJ/mol
R = Universal gas constant = 0.008314 kJ/(mol.K)
T = temperature in Kelvin
Thus, expression for rate constant at two temperatures can be written as follows:
Where, k1 is the rate constant at temperature T1 and k2 is the rate constant at temperature T2
T1 = 257oC = (257 + 273.15) K = 530.15 K
T2= 280oC = (280 + 273.15) K = 553.15 K
Thus, the factor by which rate of reaction increases i.e. ratio of K2/K1 can be written as follows:
Thus, the factor by which rate of reaction increases is 13.2
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Answer 8.
The approximate energy level diagram for catalyzed and uncatalyzed reaction can be shown as follows:
It can be seen from above diagram, the activation energy for uncatalyzed forward reaction is 101kJ/mol. The uncatalyzed reverse reaction will be endothermic reaction and its activation energy will be 198 kJ/mol as shown in above diagram.
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