A thermally activated process (a reaction) takes four minutes at 816oC. How long will it take (in minutes) at 707oC if the activation energy is 150 kJ/mol?
What is the % ionicity of the bond B_I&B_F?
To answer the first question about the time required for a thermally activated process at a different temperature, we can use the Arrhenius equation:
k = A * exp(-Ea / (R * T))
Where:
k: rate constant
A: pre-exponential factor
Ea: activation energy
R: gas constant (8.314 J/(mol*K))
T: temperature (in Kelvin)
Given that the reaction takes four minutes at 816°C (which is 816 + 273 = 1089 K), we can calculate the rate constant at that temperature by rearranging the equation:
k1 = 1 / (4 * 60) # Convert the time to seconds
Now, we can calculate the rate constant at the new temperature of 707°C (which is 707 + 273 = 980 K) using the same value of Ea (150 kJ/mol):
k2 = k1 * exp(-Ea / (R * (1/T2 - 1/T1)))
Now, we can calculate the time required at the new temperature by rearranging the Arrhenius equation once again:
t2 = 1 / (k2 * 60) # Convert the rate constant back to minutes
Substituting the values, we can calculate t2.
For the second question about the % ionicity of the bond B_I&B_F, we need more information about the bond. Please provide additional details about the bond properties, such as the nature of the atoms involved and their electron configuration.