Vocab
Steps to Finding formulas
Balancing Equations
Extra Questions
More Vocab
100
It is used to measure atoms. (It equals 1.66x10^-24 grams.)
What is atomic mass unit
100
Step 1: Obtain the mass of each element Step 2: Determine the number of moles of each type of atom present Step 3: Divide the number of moles of each element by the smallest number of moles to find the ratios. (If not all are whole numbers go to step 4) Step 4: Multiply the numbers from step three by the smallest integer that will convert all of them to whole numbers.
What is Determining the Empirical Formula
100
SnO2 + H2 → Sn + H2O
What is SnO2 + (2)H2→ Sn + (2)H2O
100
(True/False) 6.02 x 10^23 hydrogen atoms weigh 1.008g
What is false. (a mole is a counted value not measured so they don't have amu)
100
Contains 6.02 x 10^23 particles
What is a chemical mole
200
6.022x10^23
What is Avogadro's number.
200
Step 1: Balance equation Step 2: Grams to Moles Step 3: Mole Ratio to find the limiting reactant Step 4: Find the moles per product Step 5: Moles to grams
What is Solving Stoichiometry problems involving Limiting Reactants
200
Fe + H2SO4 → Fe2(SO4)3 + H2
What is (2)Fe + (3)H2SO4 → Fe2(SO4)3 + (3)H2
200
The weight of one atom of Calcium
What is 40.08amu.
200
the product that limits the amount of chemical reaction due to amount of resources
What is the limiting reactant
300
The number equal to the number of atoms of an element in the element's mass in grams.
What is mole
300
Actual Yield/ Theoretical Yield x 100%
What is Percent Yield
300
SeCl6 O2 → SeO2 + Cl2
What is SeCl6 O2 → SeO2 + (3) Cl2
300
The amount of atoms in 58.7g of Nickel
What is 6.02 x 10^23. (remember that the number of atoms is 6.02 x 10^23 because it is COUNTED)
300
Conversion factors that determine the amount of moles used to create a product or vice versa.
What is mole ratio
400
a process of using a balanced chemical equation to calculate the relative masses of reactants and products involved in a reaction.
What is stoichiometry.
400
The mass of the fraction of the product (the element) equals the mass of the element present in 1 mole of the compound divided by the mass of one mole of a compound: ex. Mass of C= 2 mol x 12.01 g/mol
What is Percent Composition
400
KNO3 + H2CO3 → K2CO3 + HNO3
What is (2)KNO3 + H2CO3 → K2CO3 + (2)HNO3
400
Find the empirical formula of C9H3
What is C3H
400
The outcome of the reactants
What is the product
500
The actual formula of a compound
What is molecular formula
500
Step 1: Balance the equation Step 2: Convert the masses/products into moles Step 3: Use the balanced equation to set up the appropriate mole ration Step 4: Use the mole ration to calculate the number of moles of the desired reactant/product Step 5: convert from moles to mass.
What is calculating the masses of reactants and products in chemical reactions (stoichiometry problems)
500
B2Br6 + HNO3 → B(NO3)3 + HBr
What is B2Br6 + (6)HNO3 → (2)B(NO3)3 + (6)HBr
500
What do coefficients in a balanced chemical equation represent.
What is quantity or ration of atoms to molecules
500
Mass in grams of 1 mole of a substance
What is its molar mass
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