Question

In: Chemistry

Considering the initial reaction above where 2 mole of SO2 react with 1 mole of O2...

Considering the initial reaction above where 2 mole of SO2 react with 1 mole of O2 to produce 2 moles of SO3, if oxygen was introduced into the system after equilibrium is reached, we would expect that (circle one) [more products would form / more reactants would form / the concentrations would not change]. If argon gas was introduced into the system after equilibrium is reached, we would expect that (circle one) [more products would form / more reactants would form / the concentrations would not change]. If the pressure is increased after equilibrium is reached, we would expect that (circle one) [more products would form / more reactants would form / the concentrations would not change].

Please explain why

Solutions

Expert Solution

In order to explain the above question we need to know the LE CHATELIER'S principle thet is If an equilibrium is subjected to strees , the equilibriun shifts in such a way to reduce the strees .

  1. In the above reaction products and reactants in the gaseous phase.so after reaching the equilibrium adding the oxygen in to the system will increase the pressure in the system.Increased pressure will convert the reatants into the product.so more product would form after the addition of oxygen in the equilibrium system, In this way the system would undo the stress after reaching equalibrium.
  2. while argon introduced in to the system would increase the pressue of the system,But the argon not involved in the reaction.so it will not cause the shift in the equilibrium.adding or removing the inert gases that not involved in the reaction would incrase the pressure but does not change the concentration of the product and reactants.

  


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