Initially:
- The student places 7 mol of ammonia in the flask, which is the initial amount of ammonia (NH3).
- The initial amount of ammonium (NH4+) is 0 mol, as there is no ammonium present at the beginning.
Change:
- The student adds 7 mol of ammonia to the flask.
- The equation for the reaction between ammonia and water to form ammonium is: NH3 (aq) + H2O (l) ⇌ NH4+ (aq) + OH- (aq)
- According to the balanced equation, the mole ratio between ammonia and ammonium is 1:1. This means that for every mole of ammonia that reacts, one mole of ammonium is formed.
- Therefore, initially, the amount of ammonia will decrease by 7 mol and the amount of ammonium will increase by 7 mol.
Equilibrium:
- At equilibrium, the concentrations of ammonia and ammonium will stabilize. The 0.2M concentration of ammonium indicates that the reaction has reached equilibrium, with some ammonia converted to ammonium and vice versa.
- At equilibrium, the amount of ammonia and ammonium will remain constant, with the forward and reverse reactions occurring at the same rate.
- The mole ratio between ammonia and ammonium, as indicated by the balanced equation (1:1), will be maintained at equilibrium.
A student places 7mol of ammonia in 14L flask. 0.2M ammonium was found in the flask. Use mole ratio to fill it the initial, change and equilibrium?
1 answer