Consider the following
N₂O₄(g)
$f$
2NO₂(g)
The equilibrium constant for this reaction will decrease with an increase in temperature.

Question

Consider the following N₂O₄(g) $f$ 2NO₂(g) The equilibrium constant for this reaction will decrease with an increase in temperature.

Quizplus · Accepted Answer

The given reaction is exothermic (producing heat), and according to Le Chatelier's principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants. However, this does not decrease the equilibrium constant; it simply shifts the position of equilibrium. The equilibrium constant, K, for a reaction is only dependent on temperature, and for an exothermic reaction, increasing the temperature actually decreases the value of K, indicating a shift in equilibrium but not a decrease in the constant itself based on the context provided. My explanation was incorrect in stating the relationship between temperature and K; increasing temperature does indeed decrease K for exothermic reactions, aligning with the original statement's implication.

Consider the Following N2O4(g) fff 2NO2(g) the Equilibrium Constant for This Reaction Will Decrease with This

Consider the Following
N₂O₄(g) $f$ 2NO₂(g)
the Equilibrium Constant for This Reaction Will Decrease with This