STEPS
What is the first step you take when doing stoichiometry?
Write the balanced equation.
What are you trying to find when you convert moles to moles?
The Mole Ratio.
What is Stoichiometry?
Mass relationships between substances in a chemical reaction.
When is 22.4 used?
When the gas is at stp.
Fe3O4 + 4 CO--->3 Fe + 4 CO2
How many moles of CO are needed to react with
16.5 g of Fe3O4?
0.285 moles CO
What is the second step you take in stoichiometry?
Start with your known substance
What are you trying to find when you convert moles to grams?
Molar Mass.
What do we look at to find mole ratios?
The coefficients in a balanced equation.
What is Avogadro's number?
6.022x10^24
How many moles of Fe2O3 will form from 5.0 moles of Fe?
2.5 moles
What is the third step you take in stoichiometry?
Covert to moles, molar ratio, or to quantity of product
What are you trying to find when you convert moles to liters in solution?
Molarity.
What is Actual Yield?
Actual amount of a product that can be formed with the limiting reactant.
How do we convert moles to grams?
Multiply by molar mass.
How many moles of KClO3 must decompose in order to produce 9 moles of oxygen gas?
6 moles KClO3
What is the last step in stoichiometry?
Check your answer makes sense!
What are you trying to find when you convert moles to liters of gas?
Molar Volume.
What is a Theoretical Yield?
The maximum amount of a product that can be given off.
What are you calculating for if you divide by 6.022x10^23 then multiply by molar mass?
Converting from particles to grams
How many grams of NaCl will be produced from 1.25 mol of chlorine gas reacting with sodium?
146 g
What is the universal language of chemistry?
Moles
Fe+O2--->Fe2O3
Find the mole ratio of Iron to Oxygen
4:3
What is Excess Reactant?
Reactant that is not used up when a reaction is run to completion.
What is multiplying molarity by volume then multiplying by 6.022x10^23?
Converting molarity to particles.
Ammonium nitrate decomposes into dinitrogen monoxide gas and water. Determine the amount in grams of water produced if 25.0 g of ammonium nitrate decomposes.
11.3grams H2O