Why is it necessary to maintain a constant temperature in an experiment to measure an equilibrium constant?

Question

Luna Chen · Accepted Answer

There is a need to maintain a constant temperature in an experiment to measure an equilibrium constant

This is only necessary for temperature related equilibrium constants not for solving #"Ka ,Kp, Kb"# but solving for #"Kc"# as a single experiment will have only one constant temperature. Different reactants will have different volume at different temperature because of the pressure will rise and for calculating Kc we sometimes need to calculate the number of moles from pressure volume and temperate which always should be a constant temperature. #"PV = nRT"# If #"T" or temperature # is not constant the #"Kc"# would be wrong. But for fall or rise in temperature the #"Kc"# values can be shown in a graph

Luna Chen · Answer

undefined Maintaining a constant temperature in an experiment to measure an equilibrium constant is necessary because temperature directly affects the equilibrium position of a chemical reaction. According to Le Chatelier's principle, if the temperature changes, the system will adjust to counteract that change. In the context of an equilibrium constant measurement, any fluctuation in temperature could lead to shifts in the equilibrium position, resulting in inaccurate or unreliable results. Therefore, by keeping the temperature constant, researchers can ensure that the equilibrium position remains stable throughout the experiment, allowing for accurate determination of the equilibrium constant.