Monitoring chemical reactions

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Question 21
Medium

Ammonium nitrate, NH4NO3\text{NH}_4\text{NO}_3NH4​NO3​, is a very common nitrogen-based fertiliser.

a.

Explain why fertilisers are important in the agricultural production of crops.

[2]
b.

Ammonium nitrate is produced by reacting ammonia with nitric acid:

NH3+HNO3→NH4NO3\text{NH}_3 + \text{HNO}_3 \rightarrow \text{NH}_4\text{NO}_3NH3​+HNO3​→NH4​NO3​

Calculate the mass of ammonium nitrate that could be made from 5.1 tonnes5.1\text{ tonnes}5.1 tonnes of ammonia.

Relative atomic masses (ArA_rAr​): H=1.0\text{H} = 1.0H=1.0, N=14.0\text{N} = 14.0N=14.0, O=16.0\text{O} = 16.0O=16.0.

[2]
c.

A student prepares some ammonium nitrate in the laboratory.

She predicts that she should make 16.0 g16.0\text{ g}16.0 g of ammonium nitrate.

Her percentage yield is 75%75\%75%.

Calculate the actual mass of ammonium nitrate that the student makes.

[2]

Monitoring chemical reactions Questions

  1. GCSE
  2. /Chemistry
  3. /Monitoring chemical reactions