Molar Mass
What is the molar mass of Fe?
55.845 g/mol
What do you use to convert from moles to moles?
Mole Ratio from a balanced chemical equation
If we combine 124.0 g of phosphorus with 176.0 g of oxygen, then what is the limiting reactant?
P + O2 -> P4O10
Phosphorus
How do I know what I need to do to convert between two things?
Identify the units and cancel the unit by putting it on the bottom.
What are the units of molar mass?
g/mol
What is the molar mass of CuO?
79.545 g/mol
Balance this equation:
CS2 + O2 -> CO2 + SO2
1, 3, 1, 2
If we combine 124.0 g of phosphorus with 176.0 g of oxygen, then what is the excess reactant? How much is left over?
P + O2 -> P4O10
Oxygen and 15.8 g
How many grams are in 5.02 x 1024 atoms of C6H12O6?
1,501 g
What is Avogadro's number?
What is the molar mass of CO2?
44 g/mol
How many moles of oxygen are needed to completely react with the carbon disulfide in the reaction above? 9.76 moles SO2
CS2 + O2 -> CO2 + SO2
14.64 moles
If 6 tanks BF3 are mixed with 3 tanks H2: What are the limiting and excess reactants?
2 BF3 + 3 H2 -> 2 B + 6 HF
BF3 is limiting
HF is excess
How many atoms are in 12 g of water?
4.013 x 1022 atoms
What is a mole?
A unit to count small quantities
What is the Molar Mass of NH4+?
18.04 g/mol
How many moles of carbon dioxide are also produced by the reaction above? 9.76 mol SO2
CS2 + O2 -> CO2 + SO2
4.88 moles
If we combine 124.0 g of phosphorus with 176.0 g of oxygen, what is the expected actual yield if the process gives a percent yield of 89.5%? [Calculate the theoretical yield and multiply by 89.5/100, or .895, to get actual yield]
P4 + O2 -> P4O10
254.3 g
What mass of iron III oxide is produced when 2.02 grams of elemental iron react with excess oxygen gas, according to the unbalanced equation:
Fe (s) + O2 (g) → Fe2O3 (s)
2.89 g
Explain the difference between limiting and excess reactants.
Limiting reactants are the reactants that run out first, and stop the reaction from continuing. Excess reactants are the ones that are left over after the reaction stops.
What is the molar mass of Al2(SO4)3?
342.15 g/mol
How many moles of carbon disulfide are needed to produce 9.76 moles of sulfur dioxide?
CS2 + O2 -> CO2 + SO2
4.88 moles
If 5.85 g HF is your calculated product and 4.63 g HF is what you actually produced, then what was your percent yield?
79.1%
Phosphoric acid, H3PO4, reacts with sodium hydroxide to produce sodium phosphate and water.
H3PO4 + NaOH -> Na3PO4 + H2O
How many grams of sodium phosphate are produced from 45.7 grams of H3PO4?
26.23 g Na3PO4
Explain the difference between actual and theoretical yield and how they interact to create the percent yield.
Actual is an amount that was produced as a product of a chemical reaction. Theoretical is the amount you should have produced that you can calculate.
Actual/Theoretical x 100