NO(g) + CO2(g)<-->NO2(g) + CO(g) delta H^degree sign = -100kJ
Which of the following will favor the forward reaction? Why?
A) add NO B) remove NO2 C) decrease the volume of the container
D) raise the temperature E) add CO
Not sure why the last posting didn't show up correctly. Hopfully this one will. D??
add heat, rxn <--
remove heat, rxn -->
To determine which of the given options will favor the forward reaction, we need to consider Le Chatelier's principle. According to this principle, if an external stress is applied to a system in equilibrium, the system will adjust itself to counteract the stress and restore equilibrium.
Let's analyze each option with respect to Le Chatelier's principle:
A) Add NO:
Adding NO to the system will increase the concentration of NO. According to Le Chatelier's principle, to counteract the increase in NO concentration, the system will shift in the direction that consumes NO. Therefore, the forward reaction will be favored.
B) Remove NO2:
Removing NO2 from the system will decrease the concentration of NO2. To restore equilibrium, the system will shift in the direction that produces more NO2. Thus, the backward reaction will be favored.
C) Decrease the volume of the container:
Decreasing the volume will increase the pressure of the system. This, in turn, will favor the side of the reaction with fewer moles of gas. In this case, the backward reaction has fewer moles of gas (1 mol) compared to the forward reaction (2 moles). Therefore, decreasing the volume will favor the backward reaction.
D) Raise the temperature:
According to Le Chatelier's principle, increasing the temperature will favor the endothermic reaction. In this case, the forward reaction is exothermic (-100 kJ), so increasing the temperature will shift the equilibrium towards the backward reaction. Thus, raising the temperature will favor the backward reaction, not the forward reaction.
E) Add CO:
Adding CO to the system will increase the concentration of CO. To counteract this increase, the system will shift in the direction that consumes CO. Therefore, the backward reaction will be favored.
Based on the analysis above, the option that favors the forward reaction is A) add NO.