The aquation of tris(1,10-phenanthroline) iron(II) in acid solution takes place according to the equation: Fe(phen) ₃²⁺ + 3 H₃O⁺ + 3 H₂O → Fe(H₂O) ₆²⁺ + 3 phenH⁺
If the activation energy,E_a,is 126 kJ/mol and the rate constant at 30°C is 9.8 × 10^-3 min^-1,what is the rate constant at 50°C?

Question

Quizplus · Accepted Answer

To find the rate constant at 50°C, we can use the Arrhenius equation which relates temperature, activation energy, and rate constant:

k2 = k1 * exp[(Ea/R) * ((1/T1) - (1/T2))]

where k1 is the rate constant at 30°C, k2 is the rate constant at 50°C, Ea is the activation energy, R is the gas constant (8.314 J/mol*K), T1 is the temperature at 30°C (303 K), and T2 is the temperature at 50°C (323 K).

Plugging in the given values, we get:

k2 = (9.8 × 10^-3 min^-1) * exp[(126000 J/mol / (8.314 J/mol*K)) * ((1/303 K) - (1/323 K))]

k2 = 2.2 × 10^-1 min^-1

Therefore, the answer is B.

The Aquation of Tris(1,10-Phenanthroline)iron(II)in Acid Solution Takes Place According to the Equation