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Determine the activation energy for the redox reaction Q²⁺ + 2 R³⁺ → Q⁴⁺ + 2 R²⁺.

Rate Constant Temperature
3.12x10^3 M^-1 s^-1 275K
2.70x10^4 M^-1 s^-1 300K

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The activation energy of the reaction is 6.1 kJ/mol.

What is the Arrhenius equation?

The Arrhenius equation specifies the relationship between the activation energy and the temperature as follows;

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

k1= 3.12x10^3 M^-1 s^-1

k2 = 2.70x10^4 M^-1 s^-1

T1=  275K

T2 = 300K

Hence;

ln(2.70x10^4/3.12x10^3) = Ea/8.314 ×(1/275 - 1/300)

2.2 = 0.0003Ea/8.314

Ea = 2.2 x 8.314/0.0003

Ea = 6.1 kJ/mol

Learn more about activation energy: https://brainly.com/question/11334504

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