what is the skeleton equation of iron(II) sulfide+ hydrochloric acid yields hydrosulfruic acid+ iron(II) chloride 2) what is the skeleton equation of potassium oxide+ water yields potassium hydroxide 3) what is the skeleton equation of ammonium sulfide+ lead(II) nitrate yields ammonium nitrate

What are the spectator ions present when aqueous solutions of rubidium phosphate and yttrium(II) bromide are mixed?

Which of the following answer choices occurs in a double replacement reaction? The reactants are two elements The reactants are two ionic compounds The products are always molecular One reactant is always oxygen

write a balanced  chemical equation based on the following iron metal reacts with oxygen gas to produce solid iron(lll) oxide

When a piece of Aluminum foil is added to an aqueous solution of hydrochloric acid, what gas is produced?       1)  oxygen gas   2)  carbon dioxide   3)  hydrogen gas   4)  chlorine gas   5)  hydrogen peroxide gas

For each of the following sets of reactants, write the balanced equation for the double displacement reaction that occurs. If you determine that a reaction will not occur, write "NR", and provide a brief explanation. Aqueous zinc chloride + aqueous sodium chromate Aqueous lithium hydroxide + phosphoric acid

1) Lead (I) nitrate reacts with sodium chloride. A) Write a balanced chemical equation to describe this reaction B) 100.0 mL of a lead (I) nitrate solution reacts with excess sodium chloride solution and produces 6.95 grams of precipitate. 2) Calculate the moles of the precipitate produced by the reaction. A) Calculate the moles of lead in the original solution. B) Calculate the molarity of the 100.0 mL lead (I) nitrate solution.

Tu Please don't provide the handwriting solution

Write the balanced molecular chemical equation for the reaction in aqueous solution for copper(1) chloride and lithium carbonate. If no reaction occurs, simply write

A chemist goes into the lab and performs an experiment in which a mixture of 8.47 grams of Zn and 6.03 g of sulfur are reacted. Before starting the experiment they perform the following calculations to predict the maximum (theoretical) yield of zinc sulfide that could be produced. First, write a balanced equation: Zn + 2 S → ZnS2 Second, check to see which reagent is limiting: 1 mole Zn 1 mole ZnS, 1 mole Zn 129.4 g ZnS, 1 mole ZnS, 8.47 g Zn × = 16.8 g ZnS, %3D 65.4 g Zn 1 mole ZnS, 129.4 g ZnS, 1 mole ZnS, 1 mole S 6.03 g S × = 12.2 g ZnS, 32.0 g S 2 moles S Since 6.03 g S produces the least amount of ZnS2, the S is limiting! They obtain an actual yield of 8.25 grams of zinc sulfide. Calculate their percent yield to one decimal place.