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Arrhenius Question

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The activation energy of a certain reaction is 32.9 kJ/mol At 25 degrees C the rate constant is 0.0160 units s-1 units. At what temperature in degrees Celsius would this reaction go twice as fast?

Given that the initial rate constant is 0.0160 s-1 at an initial temperature of 25 degrees C , what would the rate constant be at a temperature of 130 degrees C for the same reaction described in Part A?


I managed to be given the formula: ln(k2/0.0160) = (32900/0.08206)(1/298/15 - 1/403.15) but when I answered it, I got the wrong answer.

  • Arrhenius Question -

    Note that there are two questions here. The answer I gave you yesterday was for the second one. Did you report that answer for the first or the second one? Next, you simply copied what I gave you. Show your work, including the answer, and I will try to find the error.

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