PROBLEM: Dinitrogen trioxide decomposes to NO and NO2 in an endothermic process (DrH = 40.5 kJ/mol-rn). N2O3(g) < - - > NO(g) + NO2(g) Predict the effect of the following changes on the position of equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of the following changes is made. (a) adding more N2O3(g) (b) adding more NO2 (g) (c) increasing the volume of the reaction flask (d) lowering the temperature Adding more N2O3(g) will shift the equilibrium to the right Adding more NO2(g) will shift the equilibrium to the left Increasing the volume of the reaction flask will lower the pressure and favor the side with more moles of gas; therefore the rxn will shift the equilibrium to the right (d) Lowering the temperature will favor the exothermic direction; therefore, the rxn will shift the equilibrium to the left