What is the activation energy of a chemical reaction if the reaction rate triples when the temperature goes from $10^{\circ} \mathrm{C}$ to $30^{\circ} \mathrm{C}$ ?
A) $6.0 \times 10^{-20} \mathrm{~J}$
B) $7.0 \times 10^{-20} \mathrm{~J}$
C) $6.5 \times 10^{-20} \mathrm{~J}$
D) $5.5 \times 10^{-20} \mathrm{~J}$
E) $7.5 \times 10^{-20} \mathrm{~J}$

Question

Quizplus · Accepted Answer

The Arrhenius equation relates the rate of reaction to temperature and activation energy. Using the equation $k = Ae^{-\frac{E_a}{RT}}$, and given that the rate triples, we can solve for $E_a$ using the temperatures in Kelvin. The calculation shows $E_a \approx 6.5 \times 10^{-20} \mathrm{~J}$.

What Is the Activation Energy of a Chemical Reaction If 10∘C10^{\circ} \mathrm{C}10∘C

What Is the Activation Energy of a Chemical Reaction If $10^{\circ} \mathrm{C}$