2.5 mol of hydrogen sulfide gas has reacted with 1.8 mol of sulfur dioxide according to the equation:
2H2S (g) + SO2 (g)------> 3S (S) + 2H2O (l)
determine which reactant is in excess and by what mole
In the balanced equation you can see that the mole ratio of H2S to SO2 is 2:1
This means that for 2.5 mol of H2S, you would need only 1.25 mol of SO2.
Since you have 1.8 mol of SO2, it is in excess.
The amount of excess is 1.8 - 1.25 = 0.55 mol
2 H2S + SO2 -----> 3 S + 2 H2O
2 moles H2S are rquired per 1 mole SO2
1.8 moles SO2 would require 3.6 moles H2S or 2.5 moles H2S would require 1.25 moles SO2, therefore SO2 is in excess by 0.55 moles(1.8 - 1.25).
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In the balanced equation you can see that the mole ratio of H2S to SO2 is 2:1
This means that for 2.5 mol of H2S, you would need only 1.25 mol of SO2.
Since you have 1.8 mol of SO2, it is in excess.
The amount of excess is 1.8 - 1.25 = 0.55 mol
2 H2S + SO2 -----> 3 S + 2 H2O
2 moles H2S are rquired per 1 mole SO2
1.8 moles SO2 would require 3.6 moles H2S or 2.5 moles H2S would require 1.25 moles SO2, therefore SO2 is in excess by 0.55 moles(1.8 - 1.25).