Consider the following equilibrium process between dinitrogen tetrafluoride (N2F4) and nitrogen difluoride (NF2): N2F4(g) ↔ 2NF2(g) ΔH° = 38.5 kJ/mol

Which of the following changes produce more product (more NF2):

a.
Decreasing temperature.
b.
Decreasing the volume of the reacting mixture at a constant temperature.
c.
Adding a catalyst to the reacting mixture.
d.
If some N2F4 gas is removed from the reacting mixture at constant temperature and volume.
e.
If the pressure on the reacting mixture is decreased at a constant temperature.