- #1
vertciel
- 63
- 0
Hello everyone,
I am having trouble with determining where I erred in the following exercise. If someone could point out my mistake, I would appreciate the help.
Thank you!
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1. The decomposition of N2O5 has an activation energy of 103 kJ/mol and a frequency factor of [tex] 4.3E13 s^-1 [/tex]. What is the rate constant for this decomposition at 20°C?
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I simply substituted the given values into the Arrhenius Equation (omitting units to save time in typing):
[tex] k = Ae^{\frac{-E_a}{RT}}[/tex]
[tex] k = 4.3E13 \times e^{\cfrac{-103}{8.314 \times 293 K}}[/tex]
[tex] k = 4.1E13 1/s[/tex]
---
However, the given answer is:
.
I am having trouble with determining where I erred in the following exercise. If someone could point out my mistake, I would appreciate the help.
Thank you!
---
1. The decomposition of N2O5 has an activation energy of 103 kJ/mol and a frequency factor of [tex] 4.3E13 s^-1 [/tex]. What is the rate constant for this decomposition at 20°C?
---
I simply substituted the given values into the Arrhenius Equation (omitting units to save time in typing):
[tex] k = Ae^{\frac{-E_a}{RT}}[/tex]
[tex] k = 4.3E13 \times e^{\cfrac{-103}{8.314 \times 293 K}}[/tex]
[tex] k = 4.1E13 1/s[/tex]
---
However, the given answer is:
1.9E-5 1/s