If 12.5 moles of iron (II) sulfide are produced, how many moles of sulfur are needed? Round to the nearest tenth and include units.

12.5 moles

Explanation:

Given parameters:

Number of moles of FeS  = 12.5moles

Unknown:

Number of moles of sulfur needed = ?

Solution:

We have to solve from the known to the unknown using a balanced chemical equation at first.

The balanced chemical equation for this reaction is:

              Fe    +       S    →     FeS

The reaction is made possible when iron is heated in the presence of sulfur.

           we see that;

                     1 mole of sulfur produced 1 mole of FeS

                       x mole of sulfur will produce 12.5moles of iron sulfide;

Therefore, 12.5 moles of sulfur will produce that given amount of iron sulfide.

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