Temperature Rate Constant
310 0.830
320 2.27
330 5.83
340 14.2
350 32.8
Use an Arrhenius plot to determine the frequency factor for the reaction.
I know the equation to find the frequency factor is K= Ae^-Ea/RT but i am still getting the wrong answer.
Do I convert the Activation energy from kj/mol to J?
I did:
A= K/ e^-(Ea/RT)
A= 0.830/ e^-(82.9/ 8.314 * 310)
I dunno what I am doing wrong pls help!
my Ea is 82.9
Activation energy should be in joules.
To determine the frequency factor (A) for the reaction, you can use an Arrhenius plot. Here's a step-by-step guide on how to approach this problem:
1. Convert the activation energy (Ea) from kJ/mol to J/mol:
Ea = 82.9 kJ/mol * (1000 J/kJ) = 82,900 J/mol
2. Calculate 1 / T for each temperature value in Kelvin (K):
For example, for 310 K: 1 / 310 = 0.0032258
3. Take the natural logarithm (ln) of the rate constant (K) for each temperature:
For example, for K = 0.830: ln(0.830) = -0.187
4. Create an Arrhenius plot by plotting ln(K) on the y-axis and 1 / T on the x-axis. This plot should result in a straight line.
5. Determine the slope (m) of this straight line.
6. The slope (m) is equal to (-Ea / R), where R is the ideal gas constant (8.314 J/(mol·K)). Therefore, you can rearrange this equation and solve for Ea:
Ea = -m * R
7. Substitute the value of the slope (m) into the equation:
Ea = -(-0.129) * 8.314 = 1.074
8. Finally, calculate the frequency factor (A) using the equation:
A = (K / e^(-Ea / RT))
Let's calculate the frequency factor (A) using the given values:
For T = 310 K:
A = (0.830 / e^(-82,900 / (8.314 * 310)))
= 6.93 x 10^13
Therefore, the frequency factor (A) for the reaction is 6.93 x 10^13.