The following data show the rate constant of a reaction measured at several different temperatures.
Temperature (K) | Rate Constant (1/s) |
310 | 4.54×10−2 |
320 | 0.136 |
330 | 0.381 |
340 | 1.01 |
350 | 2.51 |
Part A
Use an Arrhenius plot to determine the activation barrier for the reaction.
Express your answer using three significant figures.
Part B
Use an Arrhenius plot to determine the frequency factor for the reaction.
Express your answer using two significant figures.
1/T | ln K |
0.003226 | -3.09224 |
0.003125 | -1.9951 |
0.00303 | -0.96496 |
0.002941 | 0.00995 |
0.002857 | 0.920283 |
from the plot - slope = Ea / R
so activation energy Ea = 8.314 * .10889 = 90531.15 J / mol
= 90.53 kJ / mol
now for frequency factor
lnA= intercept = 32.033
so frequency factor A = 8.2 * 1013
The following data show the rate constant of a reaction measured at several different temperatures. Temperature...
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