Answer to Question #261252 in General Chemistry for Jjj

Question

A silver metal reacts with sulfur to form silver sulfide according to the following reaction: 2Ag(s) + S(s) → Ag2S(s)

.identify the limiting reagent if 50.0 g Ag reacts with 10.0 g S

What is the theoretical yield in g of AgaS produced from the reaction?

What is the amount in g of the excess reactant expected to remain after the reaction?

When the reaction occurred, the amount of Ag-S obtained was 45.0g. What is the percent yield of the reaction?

Answer 1

2Ag(s) + S(s) → Ag2S(s)

For one mole of sulphur there should be two moles of silver for complete reaction.

Moles of silver = 50/108 = 0.46 moles

Moles of elemental sulphur = 10/32 = 0.3125 moles

For 0.3125 moles of sulphur there must be 0.6250mole of silver.

So silver is limiting Reagent.