Can anyone answer and explain this GCSE Chemistry question please?!
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Can anyone answer and explain this GCSE Chemistry question please?!

[From: ] [author: ] [Date: 12-01-29] [Hit: ]
7 tonnes of ammonia is required ( and 6.These are the relative atomic masses of each of the components of the reaction. We can see we have 17g of nitric acid + 63g of ammonia to make 80g of the fertiliser. There are 1000000g in one tonne so, we simply need to multiply it by 100000. Because we need 100000x more of the product (80x100000 = 8 tonnes).......
"Ammonium nitrate fertiliser is made from ammonia and nitric acid: NH3 + HNO3 = NH4NO3. Theoretically what mass of ammonia is needed to make 8 tonnes of ammonium nitrate? (Relative atomic masses: H = 1, N = 14, O = 16)"

If you could explain it it would be a great help, thanks :)

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Or slightly simpler.The above answer is wrong because the author has mixed up ammonia and nitric acid.

ammonium nitrate is molecular weight (Mw) 80 ammonia Mw 17

ammonium nitrate contains 17/80 = 21.3% ammonia

So 21.3% of 8 tonnes is 1.7 tonnes of ammonia is required ( and 6.3 tonnes of nitric acid)

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NH3 = 14 + (1x3) = 17
HNO3 = 1 + 14 + (16 x 3) = 63
NH4NO3 = 14 + (1x4) + 14 + (16x3) = 80
These are the relative atomic masses of each of the components of the reaction. We can see we have 17g of nitric acid + 63g of ammonia to make 80g of the fertiliser. There are 1000000g in one tonne so, we simply need to multiply it by 100000. Because we need 100000x more of the product (80x100000 = 8 tonnes). So if we need 63g of ammonia to make 80g of fertiliser, we will need (63x100000) 6300000g to make 8000000g (8 tonnes) of fertiliser. 6300000g = 6.3 tonnes
Hope that makes sense to you!
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