The substance that is NOT used up completely in a reaction.
What is the excess reactant.
100
3Fe + 4H2O --> Fe3O4 + 4H2
This mass of iron oxide is produced from 2.00mol Fe.
What is 154g Fe3O4.
100
C3H8 + 5O2 --> 3CO2 + 4H2O
This is the maximum mass of carbon dioxide produced when 0.500mol of propane (C3H8) and 3.00mol of oxygen is ignited.
What is 66.0g CO2.
100
CaO + H2O --> Ca(OH)2
A 1.50g sample of calcium oxide is reacted with an excess of water and 1.48g of calcium hydroxide is recovered. This is the percent yield in this experiment.
What is 74.8%.
100
CaO + H2O --> Ca(OH)2
This mass of calcium hydroxide is obtained from 18.7g of calcium oxide.
What is 24.7g Ca(OH)2.
200
The proportional relationship between two or more substances in a chemical reaction.
What is stoichiometry or mole ratio.
200
CH4 + 2O2 --> CO2 + 2H2O
This many liters of oxygen gas is needed to burn 10L of methane (CH4).
What is 20L O2.
200
2C4H10 + 13O2 --> 8CO2 + 10H2O
This many liters of carbon dioxide is produced when 1.00L of butane (C4H10) and 13.0L of oxygen is burned.
What is 4.00L CO2.
200
SO3 + H2O --> H2SO4
This is the percentage yield if 500.g of sulfur trioxide react with an excess of water to produce 575g of sulfuric acid (H2SO4).
What is 93.9%.
200
2Al(OH)3 --> Al2O3 + 3H2O
When 15.0g of aluminum hydroxide is decomposed, this many grams of water will be formed.
What is 5.19g H2O.
300
The measured amount of product of a reaction when the reaction is carried out in a lab.
What is the actual yield.
300
Zn + H2SO4 --> ZnSO4 + H2
This many grams of hydrogen gas will be formed from complete reaction of 6.5g of zinc with sulfuric acid (H2SO4).
What is 0.20g H2.
300
Mg + 2H2O --> Mg(OH)2 + H2
This mass of hydrogen is produced by the reaction of 4.73g of magnesium with 1.83g of water.
What is 0.102g H2.
300
2Na + Cl2 --> 2NaCl
This is the percentage yield if 200.g of chlorine react with an excess of sodium to produce 240.g of sodium chloride.
What is 72.8%.
300
N2 + 3H2 --> 2NH3
This is the maximum mass of ammonia (NH3) that can be produced by the reaction of 1.0g of nitrogen with 3.0g of hydrogen.
What is 1.2g NH3.
400
The substance that will be used up completely in a chemical reaction, and that determines the amount of product that can be made.
What is the limiting reactant.
400
2Na + Cl2 --> 2NaCl
This mass of sodium will react completely with 1.00L of chlorine gas.
What is 2.05g Na.
400
Mg3N2 + 3H2O -->2NH3 + 3MgO
This many moles of magnesium oxide are produced from the reaction of 3.82g of magnesium nitride with 7.73g of water.
What is 0.114mol MgO.
400
CH4 + 2O2 --> CO2 + 2H2O
This is the percentage yield of carbon dioxide if 1000.g of methane (CH4) react with an excess of oxygen to produce 2300.g of carbon dioxide.
What is 83.88%.
400
Cu + 2AgNO3 --> Cu(NO3)2 + 2Ag
In this reaction, 12.7g of copper produced 38.1g of silver. This is the percent yield of silver in this reaction.
What is 88.2%.
500
The maximum amount of product that can possibly be formed from the given amounts of reactants.
What is the theoretical yield.
500
C2H5OH + 3O2 --> 2CO2 + 3H2O
This volume of carbon dioxide will be produced when 0.250mol of ethanol (C2H5OH) is burned completely.
What is 11.2L CO2.
500
3AgNO3 + AlCl3 --> Al(NO3)3 + 3AgCl
This mass of silver chloride is produced when 4.22g of silver nitrate reacts with 7.73g of aluminum chloride.
What is 3.56g AgCl.
500
2Pb(NO3)2 -->2PbO + 4NO2 + O2
This is the percent yield of the decomposition reaction if 9.9g of lead (II) nitrate gives 5.5g of lead (II) oxide.
What is 82%.
500
Mg3N2 + 3H2O -->2NH3 + 3MgO
A 3.82g of magnesium nitride is reacted with 7.73g of water. The yield of magnesium oxide is 3.60g. This is the percent yield in the reaction.