For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the concentration of SO2 is doubl
Practice Questions
Q1
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the concentration of SO2 is doubled, what happens to the equilibrium constant?
It doubles
It remains the same
It halves
It quadruples
Questions & Step-by-Step Solutions
For the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g), if the concentration of SO2 is doubled, what happens to the equilibrium constant?
Step 1: Understand what the equilibrium constant (Kc) is. It is a number that tells us the ratio of the concentrations of products to reactants at equilibrium.
Step 2: Look at the reaction: 2SO2(g) + O2(g) ⇌ 2SO3(g). The equilibrium constant Kc is calculated using the concentrations of SO3 and SO2.
Step 3: Note that Kc is defined as Kc = [SO3]^2 / ([SO2]^2 * [O2]).
Step 4: Recognize that changing the concentration of SO2 (like doubling it) affects the concentrations of the reactants and products, but it does not change the value of Kc.
Step 5: Remember that Kc is only affected by temperature changes, not by changes in the concentrations of the reactants or products.
Equilibrium Constant – The equilibrium constant (Kc) is a value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature.
Le Chatelier's Principle – This principle states that if a system at equilibrium is subjected to a change in concentration, pressure, or temperature, the system will adjust to counteract that change and restore a new equilibrium.
