The reaction rate of a chemical reaction doubles when the temperature increases from 10$^{\circ}$C to 50$^{\circ}$C.What is the activation energy? A) 3.85 $\times$ 10^-20 J B) 3.33 $\times$ 10^-20 J C) 2.98 $\times$ 10^-20 J D) 2.19 $\times$ 10^-20 J E) 1.76 $\times$ 10^-20 J

Question

Quizplus · Accepted Answer

The activation energy can be calculated using the Arrhenius equation. Given that the rate doubles, the activation energy can be estimated using the formula: Ea = R * (T1 * T2 / (T2 - T1)) * ln(2), where R is the gas constant (8.314 J/mol·K), T1 and T2 are the initial and final temperatures in Kelvin. Converting the temperatures to Kelvin and substituting the values, the activation energy is approximately 2.19 * 10^-20 J.

The Reaction Rate of a Chemical Reaction Doubles When the Temperature