Consider the equilibrium reaction:
`4NH_(3((g)))+3O_(2((g)))hArr2N_(2((g)))+6H_(2)O_((g))`
`(DeltaH=-1268KJ)`
Which change will cause the reaction to shift to the right?
A. Increase the temperature
B. Decrease the volume of the container.
C. Add a catalyst to speed up the reaction.
D. Remove the gaseous water by allowing it to react and be absorbed by `KOH`.
