A reaction has an activation energy of 195.0kJ/mol. When the temperature is incr

Question

A reaction has an activation energy of 195.0kJ/mol. When the temperature is increased from 200 degrees celsius to 220 degrees celcius, the rate constant will increase by a factor of:  I know the answer is 7.5 and that you're suppose to use the Arrheinus Equation which is k = A*e^(-Ea/RT). I would like to know how you can use that one equation for solving this question. Also I would like to know where the A in the equation comes from, why it's there, and how to solve for it. Please be as detailed as possible. Thank you so so so SOOOOO much in advance.

Explanation / Answer

e ^ - 195000 J / 8.31 x 473 K = 2.85 x 10^-22

e ^ -195000 / 8.31 x 493 K = 2.13 x 10^-21

2.13 x 10^-21 / 2.85 x 10^-22 = 7.4

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