Question

A student obtained a vial of powder consisting of a mixture of iron (III) chloride hexahydrate (FeCl_3-6H_2O) and silver nitrate (AgNO_3) in unknown proportions. He weighed the vial with the powder in it and found the mass to be 20.560 g. He then poured the powder into a beaker and found the mass of the empty vial to be 15.723 g. Water was added (500 mL) to powder in the beaker, and the contents were mixed and heated for 15 minutes. Once the reaction was complete, a silver chloride precipitate was left in the water. The student then obtained a piece of filter paper with a mass of 1.043 g. put it in a funnel, and poured the contents of the beaker through it. Once the filter paper and precipitate were dried in an oven, the mass of both together was found to be 2.778 g. What was the mass of the unknown powder in the vial? Write a balanced chemical equation for the reaction that occurs between iron (III) chloride hexahydrate and silver nitrate (include phases). What is the molar mass of the following: FeCl_3-6H_2O AgNO_3 AgCl Fe(NO_3)_3 What was the mass of the silver chloride produced? How many moles of silver chloride were produced?

Answer 1

Soludion: 20.560-15.723 48378 2. Cau) h4GH,0 Ag HO3 Rgcu Fe CNo 283-15 IG9.87 1 43-32 241.85 males d Sdver elonid dca7330 0120 143.32 fui 0.0120 엉 auver c似。ride.