Chemical reaction between nitrogen monoxide and oxygen produced nitrogen dioxide.whst if the volume of the product nitrogen dioxide is being increased where will equilibrium shift to and why will it have to shift that way?
According to Le Chatelier's principle, if the volume of a reaction mixture is increased, the equilibrium will shift in the direction that produces fewer moles of gas in order to decrease the pressure. In the reaction between nitrogen monoxide and oxygen to produce nitrogen dioxide, the volume of the product nitrogen dioxide is being increased.
This means that the equilibrium will shift to the left, towards the reactants (nitrogen monoxide and oxygen), in order to decrease the pressure in the system. This is because there are more moles of gas on the reactant side of the equation (1 mole of nitrogen monoxide and 1 mole of oxygen) compared to the product side (1 mole of nitrogen dioxide).
The reaction can be represented as:
2NO + O2 ⇌ 2NO2
Therefore, if the volume of the product nitrogen dioxide is being increased, the equilibrium will shift to the left to decrease the overall pressure in the system.