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Molar Mass
Mole Conversions
Limiting/Excess and Percent Yield
Other conversions
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100

What is the molar mass of Fe?

55.845 g/mol

100

What do you use to convert from moles to moles?

Mole Ratio from a balanced chemical equation

100

If we combine 124.0 g of phosphorus with 176.0 g of oxygen, then what is the limiting reactant? 

P      +    O2   ->    P4O10

Phosphorus

100

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.

100

What are the units of molar mass?

g/mol

200

What is the molar mass of CuO?

79.545 g/mol

200

Balance this equation:

CS2 +     O2  ->    CO2   +     SO2

1, 3, 1, 2

200

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

200

How many grams are in 5.02 x 1024 atoms of C6H12O6? 

1,501 g

200

What is Avogadro's number?

6.022 x 1023
300

What is the molar mass of CO2?

44 g/mol

300

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

300

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

300

How many atoms are in 12 g of water?

4.013 x 1022 atoms

300

What is a mole?

A unit to count small quantities

400

What is the Molar Mass of NH4+?

18.04 g/mol

400

How many moles of carbon dioxide are also produced by the reaction above? 9.76 mol SO2

CS2 +     O2    ->    CO2   +     SO2

4.88 moles

400

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 

400

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

400

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. 

500

What is the molar mass of Al2(SO4)3?

342.15 g/mol

500

How many moles of carbon disulfide are needed to produce 9.76 moles of sulfur dioxide?

CS2   +     O2    ->    CO2   +     SO2

4.88 moles

500

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% 

500

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

500

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