Question
Asked Feb 12, 2020
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The rate constant of a certain reaction is known to obey the Arrhenius equation, and to have an activation energy Ea = 45.0/kJmol. If the rate constant of this reaction is 1.8 x 104·M−1s−1 at 222.0°C, what will the rate constant be at 266.0°C?

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Expert Answer

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Step 1

Given information:

Activation energy = 45.0 kJ/mol

Rate constant (k1) = 1.8×104 M-1s-1

Temperature (T1) = 222.0 °C

Temperature (T2) = 266.0 °C

Step 2

Arrhenius equation is represented as follows:

Chemistry homework question answer, step 2, image 1

 

Step 3

Since the temperature is given in degree Celsius so it would be converted into Kelvin first as follows:

Chemistry homework question answer, step 3, image 1

 

...

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