Question

A certain reaction has an activation energy of 39.5kJ/mol. As the temperature is increased from 25 degrees Celsius to a higher temperature, the rate constant increases by a factor of 6.60. Calculate the higher temperature

Answer 1

To calculate the higher temperature, we can use the equation k2/k1 = e^[(Ea/R) * ((1/T2) - (1/T1))]. Using the given data, the higher temperature is found to be 572.64°C.

Step-by-step explanation:

To calculate the higher temperature, we can use the equation:

k2/k1 = e^[(Ea/R) * ((1/T2) - (1/T1))]

Where k1 and k2 are the rate constants at temperatures T1 and T2, Ea is the activation energy, and R is the ideal gas constant (8.314 J/Kmol).

In this case, k2/k1 = 6.60, Ea = 39.5 kJ/mol, and T1 = 25°C + 273.15 = 298.15 K.

Plugging in these values, we can solve for T2:

6.60 = e^[(39.5/8.314) * ((1/T2) - (1/298.15))]

T2 = 845.79 K

Converting to degrees Celsius: T2 = 845.79 - 273.15 = 572.64°C