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If the rate of a reaction is double, when the temperature is raised from 290K to 300K, then calculate the energy of activation of it.?
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Energy of Activation Calculation:
Energy of activation (Ea) can be calculated using the Arrhenius equation:
ln(k2/k1) = Ea/R * (1/T1 - 1/T2)
Where:
- k1 is the rate constant at temperature T1
- k2 is the rate constant at temperature T2
- Ea is the energy of activation
- R is the gas constant (8.314 J/mol*K)

Given:
T1 = 290 K
T2 = 300 K
k2 = 2k1 (rate is double)

Step 1: Calculate the ratio of rate constants (k2/k1):
k2/k1 = 2

Step 2: Substitute the values into the Arrhenius equation:
ln(2) = Ea/8.314 * (1/290 - 1/300)

Step 3: Solve for Ea:
Ea = 8.314 * ln(2) / (1/290 - 1/300)

Step 4: Calculate the value of Ea:
Ea ≈ 54.38 kJ/mol
Therefore, the energy of activation of the reaction is approximately 54.38 kJ/mol.
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If the rate of a reaction is double, when the temperature is raised from 290K to 300K, then calculate the energy of activation of it.?
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