The Arrhenius equation relates the rate constant of a reaction to the activation energy, the temperature, and a constant known as the pre-exponential factor or frequency factor. The equation is given by:
k = A * exp(-Ea/RT)
where:
k = rate constant
A = pre-exponential factor or frequency factor
Ea = activation energy (in Joules/mol)
R = gas constant (8.314 J/mol-K)
T = temperature (in Kelvin)
We are given that the rate constant at 89.0°C (362.15 K) is 1.9 × 10^7 M^-1s^-1. We want to find the rate constant at 121.0°C (394.15 K).
First, we need to calculate the pre-exponential factor, A. We can do this by rearranging the Arrhenius equation and solving for A:
A = k * exp(Ea/RT)
We can plug in the values we know:
A = (1.9 × 10^7 M^-1s^-1) * exp((5.0 kJ/mol) / (8.314 J/mol-K * 362.15 K))
A = 6.46 × 10^11 M^-1s^-1
Now we can use the Arrhenius equation to calculate the rate constant at 121.0°C:
k = A * exp(-Ea/RT)
k = (6.46 × 10^11 M^-1s^-1) * exp((5.0 kJ/mol) / (8.314 J/mol-K * 394.15 K))
k = 1.9 × 10^9 M^-1s^-1
Therefore, the rate constant at 121.0°C is approximately 1.9 × 10^9 M^-1s^-1.