For a reaction, the rate constant triples when the temperature is increased from 300 K to 310 K. The activation energy (Ea) for the reaction is close to (R = 8.314 J/mol·K):
Correct: C
Using the Arrhenius equation in logarithmic form: ln(k2/k1) = -Ea/R (1/T2 - 1/T1). Given k2/k1 = 3, substituting values and solving for Ea gives approximately 46000 J/mol. The calculation involves solving the equation with the temperature difference and natural logarithm of 3.