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bekas [8.4K]
3 years ago
11

Use one of your experimentally determined values of k, the activation energy you determined, and the Arrhenius equation to calcu

late the value of the rate constant at 25 °C. Alternatively, you can simply extrapolate the straight-line plot of ln(k) vs. 1/T in your notebook to 1/298, read off the value of ln(k), and determine the value of k. Please put your answer in scientific notation. slope=-12070, Ea=100kJ/mol, k= 0.000717 (45 °C), 0.00284 (55 °C), 0.00492 (65 °C), 0.0165 (75 °C), 0.0396 (85 °C).
Chemistry
1 answer:
stealth61 [152]3 years ago
6 0

Answer:

Explanation:

Use one of your experimentally determined values of k, the activation energy you determined, and the Arrhenius equation to calculate the value of the rate constant at 25 °C. Alternatively, you can simply extrapolate the straight line plot of ln(k) vs. 1/T in your notebook to 1/298 , read off the value of ln(k), and determine the value of k. Please put your answer in scientific notation. slope=-12070, Ea=100kJ/mol, k= 0.000717(45C), 0.00284(55C), 0.00492(65C), 0.0165(75C), 0.0396(85C)

Explanation;

According to Arrhenius equation:

i.e. ln(k2/k1) = -Ea/R (1/T2 - 1/T1)

Where, k1 = 0.000717, T1 = 45 oC = (45+273) K = 318 K

T2 = 25 oC = (25 + 273) K = 298 K

i.e. ln(k2/0.000717) = -12070 (1/298 - 1/318)

i.e. ln(k2/0.000717) = -2.54738

i.e. k2/0.000717 = e^{-2.54738}

= 0.078286

Therefore, the required constant (k2) = 0.078286 * 0.000717 = 5.61*10^-^5

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