WEEK 2
You start with counting the number of atoms on the _____________ side of the yield symbol
Reactants
The atomic mass of an element, expressed in amu, is equivalent to the mass in grams of one mole of that element. True or False?
True
This is known as someones number: 6.022×10^23
Avogadro's nuber
The first step in using the mass-mass relationship to calculate the mass of a product in a chemical reaction
Convert the mass of the reactant to moles
This equations --> 2H2+O2→2H2O product is _____
Water (H2O)
Given the molar mass of a compound, you can determine how many grams are in a specific number of moles of that compound in this equation
Mass (grams)=Moles×Molar mass (g/mol)
In a mass-mass calculation, why must the balanced chemical equation be used?
It ensures that the reactants and products are properly accounted for in terms of mass.
This equation ---> 2H2+O2→2H2O) is (balanced or unbalanced)
Balanced
4 hydrogen atoms
2 oxygen atoms
A positive ion is a ____
Cation
How can you use the mole-mass relationship to determine the mass of a product in a chemical reaction?
By converting the mass of a reactant to moles, using the mole ratio from the balanced equation to find the moles of the product, and then converting the moles of the product to mass using its molar mass.
4Al+3O2→2Al2O3
The amount of grams in aluminum oxide (Al₂O₃) can be produced from 54 grams of aluminum (Al)
136g
This equation seems to be ______ (unbalanced or balanced) C2H6+O2→CO2+H2O
Unbalanced
2C2H6+7O2→4CO2+6H2O
C₆H₁₂O₆ (glucose). The formula weight of this molecule
180 g/mol
The amount of moles that are in 72 grams of carbon dioxide (CO₂)
1.64 Moles
The missing numbers for this equation __Al+__O2→___Al2O3
2, 3, 1.
H₂O (water). The formula weight of this molecule
18 g/mol
The amount of moles are in 36 grams of ammonia (NH₃)
2.12 moles