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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Step 1

Given information:

Activation energy = 45.0 kJ/mol

Rate constant (k_{1}) = 1.8×10^{4} M^{-1}s^{-1}

Temperature (T_{1}) = 222.0 ^{°}C

Temperature (T_{2}) = 266.0 ^{°}C

Step 2

Arrhenius equation is represented as follows:

Step 3

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

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