The rate constant of a reaction is 6.2 x 10^-3s-1 at 25 degrees C, and the activation energy is 33.6 KJ/mol..

What is k at 75 degrees C?

Enter your answer in scientific notation.

Use the Arrhenius equation and solve for the k needed. If you need further assistance, please explain what you don't understand about this.

To solve this problem, we can use the Arrhenius equation:

k2 = Ae^(-Ea/RT2)

Where:
- k2 is the rate constant at the new temperature T2
- A is the pre-exponential factor (which we assume to be constant)
- Ea is the activation energy
- R is the gas constant (8.314 J/(mol*K))
- T2 is the new temperature in Kelvin

First, we need to convert the given activation energy from KJ/mol to J/mol by multiplying it by 1000:
Ea = 33.6 KJ/mol x 1000 J/KJ = 33,600 J/mol

Next, we need to convert the temperatures from degrees Celsius to Kelvin:
T1 = 25°C + 273.15 = 298.15 K
T2 = 75°C + 273.15 = 348.15 K

Now we can plug the values into the Arrhenius equation and solve for k2:

k2 = (6.2 x 10^-3 s^-1) * e^(-33,600 J/mol / (8.314 J/(mol*K) * 348.15 K))

k2 ≈ 9.84 x 10^-2 s^-1

Therefore, the rate constant at 75°C is approximately 9.84 x 10^-2 s^-1.