Asked by Nk
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?
Answers
Answered by
GPT 3.5
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.
- 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.