Some Chem help please

Can someone answer this for me please? thank you =)

1) Silver sulphide and hydrogen combine to form silver and hydrogen sulphide. 3.0 g of H2 and 100 g of Ag2S are used to produce 85.0 g of Ag. The equation for the reaction is:

Ag2S + H2 -> 2Ag + H2S

A) What is the actual yield of silver?
B) Which reactant is the limiting reagent?
C) Which substance is in excess?
D) What is the theoretical yield of silver?

A) What is the actual yield of silver?
The actual yield is stated in the problem.

B) Which reactant is the limiting reagent?
3.0 g of H2 represents 1.5 moles H2.
molar mass Ag2S = 247.8 g/mol. moles Ag2S = 100 g(1 mole)/(247.8 g) = 0.40355 mole
For each mole of H2 you need 1 mole Ag2S, so Ag2S is the limiting reagent.

C) Which substance is in excess?
From the previous calculations H2 is present in excess.

D) What is the theoretical yield of silver?
Theoretical yield Ag = 0.40355 mole Ag2S(2 mole Ag(/1 mole Ag2S)(107.868 g)/(1 mole Ag)
Theoretical yield Ag = 87.06 g Ag

My hope is that you will learn the chemistry shown in the answer and not just copy it down for your homework.

Hope this is helpful to you. JIL HIR