Question

Ammonium nitrate, known for its use in agriculture, can be produced from ammonia by the following sequence of reactions - NH3(9) + O2(9) - NO(g) + H2O(g) NO(g) + O2(g) - NO2(g) NO2(g) + H2O(l) - HNO3(aq) + NO(g) HNO3(aq) + NH3(g) - NH4NO3(aq) What weight (in gm) of ammonia is required to prepare 200 gm of NH.NO: (O2 is in excess) O 106.25 63.75 42.5 51​

Answer 1

Heat =37.0 kJ when 80g NH 4 NO 3 is used.

2.50g NH 4 NO 3 produces heat of 80 (37.02.50) =1.16 kJ.

Explanation:

Answer 2

Given:

Reaction for formation of ammonium nitrate

To find:

The weight (in gm) of ammonia to prepare 200 gm of ammonium nitrate

Solution:

Balance the given equations (Attached below)

From the balanced equations, we can conclude that:

3/2 moles of ammonia react to form 1 mole of ammonium nitrate.

The molecular mass of Ammonium Nitrate = 80g

The molecular mass of Ammonia = 17g

Mass of 3/2 moles of Ammonia= 3/2 X 17 = 25.5g

∴ 25.5g NH₃ form 80g NH₄NO₃

So to form 200g NH₄NO₃,

NH₃ required = 25.5 X 200 / 80

= 63.75g (Solved using the unitary method)

Hence, 63.75g of ammonia is required.