How many moles of copper are needed to react with sulfur to produce 0.25 moles of copper(I) sulfide according to the following reaction: 2 cu + S CuS

Answer 1

Hey, this reaction is not complete, but I think we can figure it out:

Reactants:

Copper=Cu

Sulfur=S

Products (to produce Copper (I) Sulfide)

Cu₂S

So the balanced equation:

2Cu+S→Cu₂S

Note that Copper (I) Sulfide consists of:

1. Cation = Copper (I) = Cu⁺
2. Anion = Sulfide = S^2-

So if the formula is Cu₂S, the net charge is zero.

2Cu⁺+S^2-=2(+1)+(-2)=2-2=0

Now,

GIVEN: 0.25 mol Cu₂S

DESIRED: ? mol Cu

Conversion factors (from the coefficients in the balanced equation):

2 mol Cu = 1 mol Cu₂S

Factor label:

Convert mol Cu₂S to mol Cu with the coefficients:

0.25mol Cu₂S (2 mol Cu / 1 mol Cu₂S) = 0.50 mol Cu

(0.25×2÷1=0.5)