# chemistry.

What amount (in moles) of FeS2(s) are required to produced 64g of SO2(g) according to the following equation?
4FeS2(s) + 110(g)_________2FeO3(s)__8SO2(g)...remember the first long bar is an arrow.

1. 👍 0
2. 👎 0
3. 👁 1,352
1. Your equation doesn't make sense to me. I assume you mean something like this.
4FeS2 + 11 O2 ==> 2Fe2O3 + 8SO2

Convert 64 g SO2 to moles. moles = grams/molar mass.

Using the coefficients in the balanced equation, convert moles SO2 to moles FeS2.

Convert moles FeS2 to grams. grams = moles x molar mass.
Post your work if you get stuck.

1. 👍 0
2. 👎 2
2. 7.81 mol/ FeS2

1. 👍 0
2. 👎 2

## Similar Questions

1. ### CHEMISTRY

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in

2. ### chemistry

2. Ammonia is produced by the reaction of hydrogen and nitrogen. N2(g) + 3H2(g) à 2NH3(g) o a. How many moles of H2 are needed to react with 1.0 mol of N2? o b. How many moles of N2 reacted if 0.60 mol of NH3 is produced? o c.

3. ### Chem

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in

4. ### Chem

f 147 grams of FeS2 is allowed to react with 88 grams of O2 according to the following unbalanced equation, how many grams of Fe2O3 are produced? FeS2 + O2 → Fe2O3 + SO2

1. ### chemistry

Calculate the amount of energy in the form of heat that is produced when a volume of 3.56 L of SO2(g) is converted to 3.56 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C.

2. ### Chemistry

1) what mass of oxygen will react with 2.64g of magnesium? 2Mg + O2 -> MgO I was going to do 2.64g * (1/2) from the equation but im not sure. Do I have to add a 2 in front of the MgO? 2) How many moles of sodium ions are present

3. ### Chemistry

Sulfur dioxide is used to make sulfuric acid. one method of producing it is by roasting mineral sulfides, for example, FeS2(s) + O2 (g) ---> SO2(g) + Fe2O3(s) (unbalanced). A production error leads to the sulfide being placed in a

4. ### Chemistry

Consider the following mixture of SO2(g) and O2(g).If SO2(g) and O2(g) react to form SO3(g),draw a representation of the product mixture assuming the reaction goes to completion. What is the limiting reactant in the reaction? If

1. ### CHEMISTRY

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in

2. ### chemistry

suppose that you could decompose 0.250 mole of Ag2s into its elements a.How many moles of silver would you have? how many moles of sulfur would you have? b. how many moles of ag2s are there in 38.8 g of AG2S? how many moles of

3. ### Chemistry

In a reaction FeS2 is oxidized by O2toFe2O3 and SO2 . If the equivalents of O2 consumed are 'y' then the equivalents of FeS2 consumed and moles of 2 3 2 Fe O and SO produced are respectively are

4. ### Chemistry

Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in