Consider the following Equilibrium:
N2O4(g) <--> 2NO2(g) + 58.0 kJ
In what direction will the equilibrium shift when each of the following changes is made to a system at equilibrium:
a) add N2O4
b) remove NO2
c) increase the total pressure by adding N2(g)
d) increase the volume
e) decrease the temperature
N2O4(g) <--> 2NO2(g) + 58.0 kJ
In what direction will the equilibrium shift when each of the following changes is made to a system at equilibrium:
a) add N2O4
b) remove NO2
c) increase the total pressure by adding N2(g)
d) increase the volume
e) decrease the temperature
-
a) right. Adding reactant shifts towards the products.
b) right. Removing product shifts towards the products.
c) left. Increasing the pressure favors the side of the reaction with fewer moles of gas.
d) right. Increasing the volume favors the side with more moles of gas.
e) left. Reaction is endothermic as written and decreasing the temperature favors the lower energy side.
b) right. Removing product shifts towards the products.
c) left. Increasing the pressure favors the side of the reaction with fewer moles of gas.
d) right. Increasing the volume favors the side with more moles of gas.
e) left. Reaction is endothermic as written and decreasing the temperature favors the lower energy side.