Part II (76 points total): Carefully show your work so that, if necessary, parti
ID: 304129 • Letter: P
Question
Part II (76 points total): Carefully show your work so that, if necessary, partial credit may be determined and awarded. Where appropriate, be sure to indicate units! For each of the following stresses, indicate whether the reaction would shift to the right, shift to the left, or if the stress would not cause a shift. Also tell whether the value of Keq would go up, down, or remain the same. (12 pts) 2SO2 (g) + O2 (g) ? 2S03 (g) ??? =-99 kJ a. Addition of SO2 (g) b. Increasing the volume of the container at a constant temperature. c. Increasing the temperature of the reaction mixture.Explanation / Answer
This can be clearly and nicely explianed by Le Chetelier principle.
According to this principle if a equilibrium is disturbed by something then the position of the equilibrium shifts in such direction to counteract the change.
As from the given reaction it is clear that we started with 3 mole of reactants and finally we obtained 2 mole of products. So the volume is decreasing during the reaction.
a. As you are adding SO2 from outside the moles of SO2 will increase and it will increase the pressure of reactants side. So according to this priinciple the equilibrium should shift in such a direfction where the pressure is lesser. So clearly the reaction quilibrium will shift towards right.
b. As at a constant temperature we are increasing the volume of the container, that decreases the pressure of the container. So the reaction equilibrium will shift in such a direction where the pressure is more. So the equilibrium will shift towards left as there are more number of reactants i.e pressure is more on that side.
c. As from the change of enthalpy value it is clear that the reaction is exothermic. So if we increase the temperature of the system the equilibrium will shift towards left as the temperature is less on the reactants side for the exothermic reaction.