Reaction ID
This is the reaction type for P4 + 6F2 -> 4PF3, where two substances form one.
Combination
In the formula 6F2, this is the total number of individual atoms of Fluorine represented.
12 (6*2)
These ions appear on both sides of a chemical equation and are "canceled out" to find the net ionic equation.
spectator ions
In the equation P4 + 6F2 -> 4PF3, this is the mole ratio between Phosphorus (P4) and Fluorine (F2).
1:6
To find this, you divide your "Actual Yield" by your "Theoretical Yield" and multiply by 100.
% yield
The reaction 2NaN3 -> 2Na + 3N2 belongs to this category because one substance breaks into two.
Decomposition
In the equation 4PF3 (g), the (g) tells the chemist that the product is in this physical state.
gas
This is the term for a solid, insoluble product that forms during a double-replacement reaction.
precipitate
If you react 3 moles of P4 with excess Fluorine, this is the total number of moles of 4PF3 produced.
12 (3*4)
In the reaction of NO2 and H2O, if you have 15 moles of NO2 and 6 moles of H2O, this reactant will run out first.
3NO2 + H2O -> NO + 2HNO3
15 mole NO2 / 3 = 5 mole NO2
6 mole H2O / 1 = 6 mole H2O
NO2 is the limiting reactant
This specific type of reaction always involves a hydrocarbon reacting with Oxygen to produce CO2 and H2O.
Combustion
In a chemical equation, what are these large numbers (like the 6 in 6F2) that tell you how many moles of a substance are used called?
coefficients
A reaction where two parts of two ionic reactants switch places to form two new products is known as this.
Double Replacement
This is the term for the reactant that is completely consumed first and stops the reaction.
limiting reactant
This law explains why we must balance equations: "Mass is neither created nor destroyed."
Law of Conservation of Mass
2K + 2H2O -> 2KOH + H2 is an example of this reaction type, where one element kicks out another.
Single Replacement
This "bones only" version of an equation shows the formulas of reactants and products but is not yet balanced.
skeleton
This type of equation shows dissolved ionic compounds as dissociated free ions (e.g. Ag+ + NO3-) with the spectator ions.
Total ionic equation
This is the amount of reactant that remains after the limiting reactant has been completely used up.
excess reactant
Calculate the molar mass of Nitric Acid (HNO3) using H=1, N=14, O=16.
H- 1 x 1 =1
N- 14 x 1 =14
O- 16 x 3 =48
63g/mol
Ca(OH)2 + 2HCl -> CaCl2 + 2H2O is this specific type of reaction
Double Replacement
When balancing an equation, you are permitted to change coefficients, but you must never change these.
subscripts
The equation that has the spectator ions removed is called the...
net ionic equation
If your theoretical yield is 500g but you only produce 490g in the lab, this is your percent yield.
(490 / 500) * 100% = 98%
Balance this: NO2 + H2O -> NO + HNO3.
3NO2 + H2O -> NO + 2HNO3