What is the effect of increasing temperature on the rate constant (k)?

The rate constant increases exponentially as temperature increases. 


For many reactions, the rate constant doubles for each 10°C rise in temperature.

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State and explain the effect of increasing temperature on the rate of reaction.

As temperature increases, the rate of reaction increases.


This is because:

  1. At higher temperatures, molecules move faster, resulting in more frequent collisions.
  2. At higher temperatures, molecules have greater kinetic energy, allowing a higher proportion to exceed the activation energy barrier.

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What is the Arrhenius equation?

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k = Ae(RT−Ea​​)


k = rate constant

A = pre-exponential factor

Ea = activation energy (kJ mol-1)

R = gas constant (J K-1 mol-1)

T = temperature (K)

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What is the logarithmic form of the Arrhenius equation?

ln(k)=−RTEa​​+ln(A)

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What information does the gradient and y-intercept of an Arrhenius plot tell you?

Gradient =−REa ​​
y−intercept =ln(A)

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Explain why a small increase in temperature results in a large increase in rate of reaction.

A small increase in temperature results in a significantly higher fraction of molecules having energy greater than, or equal to, the activation energy. This means a much higher proportion of collisions are successful and the rate of reaction increases by a large amount.

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