# Stoichiometry

How much iron (II) sulfide would be needed to prepare 15L of hydrogen sulfide? My balanced equation is 2HCl + FeS --> H2S + FeCl2. I have converted 15L H2S to mols, but I have no idea where to go from here.

1. 👍
2. 👎
3. 👁
1. You're half way there IF the H2S is at STP. If not then an adjustment needs to be made.
But let me start over to make sure we don't miss something. Here are the general steps (assuming STP conditions for the H2S).

Step 1. Write the balanced equation. You have done that.
2HCl + FeS ==> H2S + FeCl2

Step 2. Convert what you have into mols. You have done that.
15L H2S x (1 mol H2S/34 g H2S) = 0.441 mol H2S.

Step 3. Using the coefficients in the balanced equation, convert mols of what you have (in this case H2S) to mols of what you want (in this case mols FeS).
mols FeS = 0.441 mols H2S x (1 mol FeS/1 mol H2S) = 0.441 mol x 1/1 = 0.441 mol FeS

Step 4. Now convert mols FeS to grams.
grams = mols FeS x molar mass FeS.

This procedure will work most stoichiometry problems.
Check my arithmetic. I estimated the molar mass of H2S so you need to redo that part and follow through.

1. 👍
2. 👎

## Similar Questions

1. ### chemistry

Write the net ionic equation for the precipitation of iron(II) sulfide from aqueous solution:

2. ### Chem 1010

Aqueous solutions of sodium sulfide and silver nitrate are mixed to form solid silver sulfide and aqueous sodium nitrate. The complete ionic equation contains which one of the following terms (when balanced in standard form)?

3. ### CHEMISTRY

2H2S + 3O2 → 2H2O +2SO2 given the balanced equation, if 4 moles of hydrogen sulfide react: How many moles of oxygen consumed? How many moles of water and sulfur dioxide are produced?

4. ### chemistry

Will sodium sulfide and iron II sulfate form a precipitate? if so what would the reaction look like?

1. ### chemistry

hydrogen sulfide gas is bubbled through a solution of iron III chloride state and explain what happens

2. ### Chem Help!

I really need help for my homework on how to write the balanced equation for the following reactions. 1) Sodium reacts with iron(lll)oxide to produce sodium oxide and iron. Type of reaction: Balanced Equation: 2) Hydrogen bromide

3. ### chemistry

aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide a. balance the chem eqn for this rxn Al2S3+6H2O = 2Al(OH)3+3H2S b.how many g of water are needed in the rxn to produce al(oh)3? what is the formula

4. ### Chemistry

Magnetite, an iron ore with formula Fe3O4, can be reduced by treatment with hydrogen to yield iron metal and water vapor. (a) Write the balanced equation. (Use the lowest possible coefficients.) 1Fe3O4(s) + 4H2(g)-> 3Fe(s) +

1. ### chemistry

write a balanced chem equation for solid lead (II) sulfide reacts with aq hydrochloric acid to form solid lead (II) chloride and dihydrogen sulfide gas.

2. ### URGENT! chemistry- percentage yield

heating an ore of antimony sulfide in the presence of iron gives th element antimony and iron(2) sulfide. when 15.0 antimony sulfide reacts with an excess of iron, 9.84 g antimony is produced. what is the percent yield of this

3. ### science

When hydrochloric acid reacts with sodium sulfide, hydrogen sulfide gas and sodium chloride are produced. How many moles of H2S will be generated by 2.56 moles of HCl? 2HCl + Na2S → H2S + 2NaCl

4. ### chemistry

sodium sulfide and cadmium nitrate undergo a double displacement reactions as shown by the following equation Na2S cd(NO3)2 -> 2NaNO3 CdS What is the mass, in milligrams,of cadmium sulfide that can be made from 5.00mg of sodium