The Student Room Group

OCR A Chemistry question? Set 2 Paper 1

I can't screenshot the question so I will type it out.

Much of the sulfur required for the production of sulfuric acid is obtained from sulfur impurities in natural gas, such as hydrogen sulfide, H2S.

The H2S is converted into Sulfur in two steps.

1: Some of the H2S is reacted with oxygen to form sulfur dioxide, SO2.

2H2S (g) + 3O2 (g) -> 2SO2 (g) + 2H2O (g)

Step 2: The remaining H2S is reacted with SO2 to produce sulfur.

2H2S(g)+ SO2 (g)-> 3S(s) + 2H2O(g)

Construct the overall equation for the two steps below.

Answer: 2H2S(g) + O2(g) -> 2S(s) + 2H2O (g)

Methodology please?
Reply 1
The second equation only uses 1 mole of SO2, whereas 2 moles are made in the first reaction. Double the moles of the second equation then find the overall by adding reactants to reactants and products to products, cancelling anything that is on both sides. Also simplify the multiples, although they mark would probably be given if left with multiples.

Quick Reply

Latest