Balancing
Name for numbers used to balance a chemical equation
Coefficients
a way to measure elements
Stoichiometry
2 K + 2 H2O → 2 KOH + H
Each mole of K requires ____ moles of H2O
1 mole H2O
Units of molarity
Molar (M) = mol / L
A homogeneous mixture of a solute in a solvent
Solution
H2 + O2 → H2O
2 H2 + O2 → 2 H2O
Used to convert between grams and moles of a compound.
Molar Mass (add masses from periodic table)
What is the limiting reactant?
H2 + Cl = 2HCl
H= 4.00 mol
Cl= 2.00 mol
Cl
Molarity of 0.5 mol of NaCl in 1 L of solution
0.5 M NaCl
The lesser amount, dissolved in a solution
Solute
P4O10 + H2O → H3PO4
P4O10 + 6 H2O → 4 H3PO4
The only way to covert from one compound to a DIFFERENT compound.
Mole Ratio
Calculate the % yield if 75g of product is weighed for a reaction with a theoretical yield of 100g.
(75g)/(100g) * 100 = 75%
Equation to calculate total volume needed to dilute a concentrated solution to a given lower molarity.
M1V1 = M2V2
Dissolves the solute in a solution
Solvent
The synthesis of Iron (III) Chloride
2 Fe + 3 Cl2 → 2 FeCl3
Starting quantity that is used up in a reaction first
limiting reactant
C4H10 + 13 O2 --> 8 CO2 + 10 H2O
Given: 2.46g H2O
Unknown: ? moles C4H10
0.0137 moles C4H10
If 97.0 mL of a 1.30 M solution of LiCl is diluted to 150 mL, determine the concentration of the new solution.
0.841 M LiCl
Name for a solution when the solvent is water.
Aqueous
Aluminum reacts with hydrochloric acid (HCl)
2 Al + 6 HCl → 2 AlCl3 + 3 H2
The maximum amount of product possibly formed
Theoretical (Expected) Yield
2 Al + 6 HCl --> 2 AlCl3 + 3 H2
Given: 16.5g Al
Unknown: ?g AlCl3
81.5g AlCl3
The mass of solute given a solution containing 725 mL of .25 M (NH4)2SO4
[HINT: Molar mass = 132.14 g/mol]
24 grams (NH4)2SO4
Solution after adding significant volume of solvent to a concentrated sample.
Dilute solution (lower molarity)