# How much ammonia is required to produce 1 kg of standard ammonium nitrate containing 96%

**How much ammonia is required to produce 1 kg of standard ammonium nitrate containing 96% ammonium nitrate?**

NH3 + HNO3 = NH4NO3

First, let’s calculate the mass of pure ammonium nitrate

m (NH4NO3) = m (total) * w (NH4NO3) = 1000 * 0.96 = 960 g.

where, 1kg = 1000 gr., and 0.96 – 96% is the content of nitrate

Under the conditions of the problem, it is not said under what conditions the reaction occurs, so we will take them as normal conditions.

Under normal conditions, 1 mol of any gas occupies a molar volume of 22.4 l / mol. It can be seen from the reaction equation that from 1 mol of NH3, 1 mol of NH4NO3 is obtained.

Let’s make the proportion:

X / 22.4 = 960/80

Where M (NH4NO3) = 14 + 4 * 1 + 14 + 3 * 16 = 14 + 4 + 14 + 48 = 80 g / mol

a X is the required volume of ammonia

whence X = (22.4 * 80) / 960 = 1.87 liters.

Answer: the volume of ammonia is 1.87 liters.