For a gas-phase reaction where the total moles of gaseous reactants equals the total moles of gaseous products, what happens when the total pressure is increased?
Answer
The equilibrium position does not shift.
Pressure changes only cause a shift if there is a difference in the total number of moles of gas between the reactant and product sides. If the mole count is equal, increasing total pressure has no effect on the equilibrium position.
#Videos
Le Chatelier's Principle
Related Questions
What condition defines a state of chemical equilibrium?How is the equilibrium constant ($K$) mathematically derived for a generic reaction A $
ightleftharpoons$ B?If the equilibrium constant ($K$) for a reaction is very large ($K
ot extgreater
ot extgreater 1$), what does this imply about the system at equilibrium?Which external variable is the only one mentioned that actually changes the intrinsic value of the equilibrium constant ($K$)?What is the name given to the principle that predicts how an equilibrium system will adjust to an applied external stress?If a system at equilibrium has additional reactant added, how does the system respond to re-establish balance?What is the primary effect of introducing a catalyst into a reaction mixture that is currently at equilibrium?For a gas-phase reaction where the total moles of gaseous reactants equals the total moles of gaseous products, what happens when the total pressure is increased?In an exothermic reaction, what effect does increasing the temperature have on the equilibrium position?If a desired product formation reaction is endothermic, what happens to the equilibrium constant ($K$) if the temperature is raised?If a reaction has an equilibrium constant ($K$) that slightly favors the reactants ($K<1$), what strategy can a chemist use to ensure a high yield of product?