Conceptual
A + B --> C + D
If you combine 10g of A with 20g of B and produce 5g of C, how much D did you produce?
25g of D
Law of Conservation of Mass
You are creating a compound made of sodium and nitrite. What is its chemical formula?
NaNO2
4Fe + 3O2 --> 2Fe2O3
You start with 12 grams of Fe and excess O2. How many moles of iron(III) oxide do you produce?
0.11 mol Fe2O3
A + B --> C + D
According to the following information, which reactant will RUN OUT first (be used up)?
200g of A theoretically yields 50g of D
30g of B theoretically yields 80g of D
A will run out first
What do you call the amount of a substance that is made in the lab, and what do you call the amount of a substance that SHOULD react or be produce according to stoichiometry?
Actual (yield, mass, amount)
Theoretical (yield, mass, amount)
What conversion factor will ALWAYS be used during stoichiometry?
Mole ratio
You produce 5 moles of CO2 during a reaction. What volume does this take up at STP?
100 L
4Fe + 3O2 --> 2Fe2O3
You want to use 4 moles of O2. How many grams of iron(III) oxide will you produce?
426.5g Fe2O3
With sigfigs 400g Fe2O3
A + B --> C + D
If B is a limiting reactant, after the reaction, which could be possible depending on the starting mass of A? (select all)
A: A is used up entirely
B: There is not enough A to react completely with B
c: There is some A leftover
A and C
What is the equation for percent yield?
%Yield = (actual/theoretical) x 100%
2NaOH --> Na2O + H2O
What is the ratio of sodium hydroxide to sodium oxide?
2 mol NaOH / 1 mol Na2O
Write a skeletal equation for the following word equation:
Aqueous sodium hydroxide reacts with aqueous hydrochloric acid (hydrogen monochloride) to produce water and a soluble salt.
NaOH(aq) + HCl(aq) --> H2O(l) + NaCl(aq)
C3H8 + 5O2 → 3CO2 + 4H2O
What mass of water can you make by combusting 27.0g C3H8?
44.1g H2O
What is the limiting reactant if you start with 10g of each reactant in a reaction where hydrogen gas reacts with oxygen gas to produce water?
Oxygen gas
CH4 + 2O2 --> CO2 + 2H2O
If you used 20g of CH4 to create 10g of CO2 according to the balanced equation above, what was your percent yield of CO2?
Molar masses: (CH4: 16.04) (CO2:44.01)
18.2%
With sigfigs: 20%
If you are trying to convert from mass to moles using a molar mass of 12.01g/mol, what goes on the top of the conversion factor, and what goes on the bottom? Write as a fraction.
1 mol / 12.01g
Balance the following equation:
TiCl4 + O2 → TiO2 + Cl2
TiCl4 + O2 → TiO2 + 2Cl2
C3H8 + 5O2 → 3CO2 + 4H2O
What volume of CO2 can you produce by combusting 1.5050E24 atoms of C3H8 at STP?
170.25L CO2
3NaOH+H3PO4→Na3PO4+3H2O
14g of NaOH react with 12g of H3PO4 to produce sodium phosphate and water. What is the maximum mass of Na3PO4 that can actually be produced?
19.2g Na3PO4
CH4 + 2O2 --> CO2 + 2H2O
Your percent yield of water was 60% after creating 30.0g of water in the lab. What mass of oxygen gas was used during this reaction?
88.6g oxygen