Question

0.5 mol of each H2S and SO2 are mixed together in a reaction flask in which the following reaction takes place; calculate the number of moles of sulphur formed. 2H2S(g) + SO2(g) -------> 2H2O(l) + 3 S(s). Solution states in answer to divide by 4. Provide the reasoning behind it

Answer 1

2 H2S  + SO2  ===>   2 H2O  + 3 S

So 2 moles of H2S reacts with 1 mole of SO2.  
We have 0.5 moles of H2S and SO2.  Then  0.5 moles of H2S reacts with 1/4 moles of SO2, and forms 2/4 =1/2 moles of water and   3/4 moles of Sulfur.

So answer =  3/4 moles.

Answer is :   if 2 moles of H2S forms  3 moles of S, then 1/2 mole of H2 forms  3/4 mole of S.

If we take SO2 , o.5 moles will require  1 mole of H2S to completely react. So SO2 does not consume totally.  H2S is consumed totally.

Answer 2

Answer:

here is ur short answer