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Stoichiometry: Relationship between reactions and products in equations…
Stoichiometry: Relationship between reactions and products in equations
Percent Yield:
calculated by dividing the experimental yield by the theoretical yield and multiplying by 100%
Example: Actual Yield (29 g CO2)/Theoretical yield x 100 (36.7g C02) = 29/36.7= 0.79= 79%
Use: Chemical reactions very often form by-products as well as the intended product. in most reactions, not all of the reactants actually react.
Theoretical Yield: the theoretical amount of a substance produced in a chemical reaction.
Actual Yield: the
actual
amount of a substance produced in a chemical reaction
Limiting Reactions: The amount of the reactant that is limiting the amount of the product produced
Example: C+0=CO
Use: It tells the chemists how much of a substance is needed.
Excess Reactants: A reactant in a chemical reaction with an excess amount of the substance, which is more than necessary to complete the reaction.
Mole:
the mass of substance containing the same number of fundamental units as there are atoms in exactly 12.000 g of 12C
Mole Ratios:
The mathematical relationship between 2 species in a chemical reaction
The mathematical relationship between 2 species in a chemical reaction
a
species
is a chemical substance or ensemble composed of chemically identical molecular entities that can explore the same set of molecular energy levels on a characteristic or delineated time scale
Molar mass of elements vs. compounds
Molar mass of elements: the mass in grams of 1 mole of particles
Example: Na=22.99g
Use: Count the number of particles by massing the substance
Molar mass of compounds: Atomic mass times the number of elements in the equation
Use: Count the number of particles in a compound by massing them
Example: H2O=6.02x10^23 molecules of water= 18.02 grams
"Little Map"
mapped relationship between units of stoichiometry (same element or compound)
Use: Converting units between moles, mass, volume, and particles.
Example: Moles to Mass (1 step), Mass to Volume (2 steps)
"Big Map": mapped relationship between units of stoichiometry (different elements/compounds)
Example: Moles to Moles
Use: to convert mass/volume/particles/moles of one element/compound to that of another
Molar Volume: the volume occupied by one mole of ideal gas at STP
Example: Helium Gas molar volume- 6.8L
STP: Standard Temperature & Pressure (0K, 1 Atmosphere)
Use: to find the volume occupied by one mole of gas at standard temperature and pressure
Coefficient: The number appearing before each symbol in a reaction
Use: to tell how many of a specific molecule are present in a chemical reaction
Example: 2Na; coefficient is 2
Significant Figures: the numbers in a scientific calculation that are used to display the most accuracy
Rule 3: Leading zeros are not significant
Rule 1: Non- zero numbers are significant.
Rule 2: Captured zeros are significant
Rule 4: Trailing zeros are significant if there is a decimal place anywhere
Equimolar: Substances with the same amount of moles
Example: 2 substances with the same amount of moles