Given that the initial rate constant is 0.0190s^-1 at an initial temperature of 20 degrees Celsius, what would the rate constant be at a temperature of 170 degrees Celsius?
Activation energy = 45.2kJ/mol
I kept on getting 1.13s^-1 as my value for k2 but it's wrong...
To determine the rate constant at a different temperature, we can use the Arrhenius equation, which relates the rate constant (k) to the temperature (T) and the activation energy (Ea):
k = A * e^(-Ea / (R * T))
where:
- k is the rate constant
- A is the pre-exponential factor (often given for a specific reaction)
- Ea is the activation energy
- R is the gas constant (8.314 J/(mol·K))
- T is the temperature in Kelvin (K)
Given:
- Initial rate constant (k1) = 0.0190 s^(-1) at an initial temperature (T1) = 20 degrees Celsius
- Activation energy (Ea) = 45.2 kJ/mol
Now, we need to convert the temperatures to Kelvin:
- T1 = 20 + 273.15 = 293.15 K
- T2 = 170 + 273.15 = 443.15 K
Next, we can plug in the values into the equation and solve for k2:
k2 = A * e^(-Ea / (R * T2))
To calculate k2, we need the value of A (pre-exponential factor). If you have that value or any additional information, please provide it and I can help you further.