What is true about the reaction quotient (Q) when Qp is less than Kp?

When the reaction quotient ( Q_p ) is less than the equilibrium constant ( K_p ), it indicates that the reaction is not at equilibrium and will shift to the right. This is because the system will favor the formation of products in order to increase the value of ( Q_p ) until it equals ( K_p ).

At equilibrium, ( Q_p ) equals ( K_p ), which corresponds to a balance between the concentrations or partial pressures of reactants and products. When ( Q_p ) is less than ( K_p ), it means that there are not enough products relative to reactants present at this moment in the reaction, prompting the system to move toward the products and decrease the concentration of reactants.

Thus, the correct interpretation is that the reaction is moving from left to right. This shift will continue until the equilibrium condition is met, at which point ( Q_p ) will equal ( K_p ). Overall, this understanding is crucial in predicting how a chemical system will respond to changes in concentration or pressure, thus aiding in thermochemical calculations and insights.