What is the effect of temperature on K(equilibrium constant)?
For this question we need to consider the equation:
ΔStotal = ΔSsystem - ΔH/T
For and exothermic reaction, -ΔH/T is positive. Therefore, as T increases -ΔH/T becomes more negative, ΔStotal becomes less positive/more negative and the position of equilibria moves to the left. This results in K decreasing.
For an endothermic reaction, -ΔH/T is negative. Therefore, as T increases, -ΔH/T becomes less negative, ΔStotal becomes less negative/more positive and the position of equilibrium moves to the right. This results in K increasing.
OP
Related Chemistry A Level answers
All answers ▸State why it is initially unexpected for alkenes to undergo electrophilic addition with bromine. Explain why this reaction does indeed occur.
Explain why transition metal compounds are often coloured in solution.
What is clonal selection?
Using your knowledge of periodicity and atomic structure, why does the first ionisation energy decrease moving down a group yet increase moving along a period in the periodic table?