Given the unbalanced reaction, Fe + S > Fe S , how 8 2 3
many moles of each reactant are needed to produce 1.50 moles of iron (III) sulfide? (balance equation first)

The answer to your question is 3 moles of Fe and 4.5 moles of S

Explanation:

Data

moles of Fe = ?

moles of S = ?

moles of Fe₂S₃

Unbalanced chemical reaction

                    Fe   +  S   ⇒    Fe₂S₃

             Reactants    Elements    Products

                     1                  Fe                2

                     1                   S                 3

Balanced chemical reaction

                    2Fe   +  3S   ⇒    Fe₂S₃

             Reactants    Elements    Products

                     2                  Fe                2

                     3                   S                 3

-Calculate the moles of each reactant

                  2 moles of Fe 1 mol of Fe₂S₃

                 x                       1.5 moles Fe₂S₃

                               x = (1.5 x 2) / 1

                                x = 3 moles of Fe

-Calculate the moles of S

                  3 moles of S 1 mol of Fe₂S₃

                  x                     1.5 moles of Fe₂S₃

                                x = (1.5 x 3) / 1

                                x = 4.5 moles of S

sodium (na), for example, has one electron in its valence shell. this is an unstable state because that valence shell needs eight electrons to be full. in order to fill its valence shell, find a way to add seven electrons to its valence shell

a non redox reaction occurs when there is not a transfer of electrons. for redox reactions, which are reduction-oxidation reactions, a change in the oxidation number occurs. elements that are reduced gain electrons, and elements that are oxidized lose electrons.

explanation: