[Shordaay]

could someone please help me with these questions please.. also could you explain how you got the answer...

1. N2 (g) + 3H2 (g) --> 2NH3

(i)what volume of hydrogen (R.T.P) is needed to react exactly with 2.8kg of N2?
(ii). what mass if ammonia would be produced assuming that r*n was complete?
(iii). what mass of ammonium nitrate fertilizer could be made from this amount of ammonia?

2. copper (II) nitrate can be prepared by adding copper(II) oxide to nitric acid. what is the maximum mass of copper (II) nitrate which can be formed from 150cm3 of nitric acid of concentration 0.5mol/dm-3?

3. what mass of potassium hydrogen carbonate must be added to sulphuric acid to produce 8.7g of potassium sulphate?

4. 50cm3 of an acid with formula HnX and concentration 0.4mol/dm-3 are needed to neutralize 100cm3 of potassium carbonate solution of cone 13.8g/dm-3. calculate the value of n in HnX.

[clownfish]

(Original post by Shordaay)
could someone please help me with these questions please.. also could you explain how you got the answer...

1. N2 (g) + 3H2 (g) --> 2NH3

(i)what volume of hydrogen (R.T.P) is needed to react exactly with 2.8kg of N2?
(ii). what mass if ammonia would be produced assuming that r*n was complete?
(iii). what mass of ammonium nitrate fertilizer could be made from this amount of ammonia?

2. copper (II) nitrate can be prepared by adding copper(II) oxide to nitric acid. what is the maximum mass of copper (II) nitrate which can be formed from 150cm3 of nitric acid of concentration 0.5mol/dm-3?

3. what mass of potassium hydrogen carbonate must be added to sulphuric acid to produce 8.7g of potassium sulphate?

4. 50cm3 of an acid with formula HnX and concentration 0.4mol/dm-3 are needed to neutralize 100cm3 of potassium carbonate solution of cone 13.8g/dm-3. calculate the value of n in HnX.

In all cases you need to get into moles:

If you are given a mass, then use moles = mass/molar mass

If you are given a solution, then use moles = concentration x volume (if volume is in cm3 then you need to divide by 1000 to get it into dm3)

If you are given a gas, then use moles = volume (in dm3)/24


Once you are in moles, use the molar ratio (which you get from the chemical equation) to find the number of moles of what you are interested in. Then use one of the equations above to get it into the format (mass, volume, concentration) that you want.

I'll leave you to try them rather than write the answers etc.

[Shordaay]

thank you for your help

[desslop]

i. n=m/mr
= 2800/14
= 200 moles of Nitrogen
Reacting ratio = 1 Nitrogen Atom to 3 Hydrogen Atom
Hence there are 200*3 moles of Hydrogen which is 600 Moles
n=v/24
v=n*24
= 600*24
= 14000 cm cubed
= 14 dm cubed

Work out the rest yourself