The Mole
A unit in chemistry used to count atoms and molecules.
The mole
The molar mass of sodium (Na)
22.99
This describes how to convert from grams to moles.
Divide by molar mass.
A s'mores recipe that calls for 2 graham crackers, 1 chocolate and 1 marshmellow would require this many graham crackers to make 50 s'mores.
100 graham crackers
Coefficients in a chemical equation are also known as these.
Mole values
This number was named after Avogadro and represents 1 mole of anything.
6.022x10^23
The unit for molar mass.
Grams per mole or g/mol
This describes how to convert from # atoms (or molecules) to moles.
Divide by 6.022x10^23
Stoichiometry is the relationship between these two quantities in a chemical reaction.
Quantities of reactants and products.
When making a grilled cheese, if I have 4 slices of bread and 3 pieces of cheese, this ingredient limits the amount of sandwiches I can make.
Bread
The mole is similar to a dozen or another counting number in this way.
It represents an amount (6.022x10^23) of items.
This process describes how to calculate molar mass for a compound.
Find the atomic mass of each element, multiply mass by the element's subscript, and add all masses together.
True or false: there is a direct conversion step between #atoms and grams.
False.
In the formation of water: 2H2 + O2 --> 2H2O, if I begin the reaction with 7 moles of O2, I would make this many moles of water.
14 moles of water
Percent yield is used in chemistry to determine this.
How much product was produced in a chemical reaction compared to how much was expected to be produced.
Between gold and silver, this substance weighs more.
Gold (larger atomic mass)
The molar mass of C3H5OH
58.09 g/mol
The number of moles in 78 grams of NaOH
1.95 moles of NaOH
In the formation of water, if I begin the reaction with 100 grams of H2, this is how many moles of water I will make.
49.50 moles of water
In the formation of water, If i begin the reaction with 7 moles of H2 and 3 moles of O2, my limiting reactant would be this.
O2 (7 moles H2 produces 7 moles of water and 3 moles O2 produces 6 moles of water)
True or false: a mole of gold and a mole of silver would contain the same amount of particles.
True
The molar mass of (NH4)3PO4
149.09 g/mol
The number of grams in 3.5x10^23 molecules of C6H12O6
104.50 grams of C6H12O6
Given 50 grams of oxygen for the formation of water, this is how many grams of water could form.
56.22 grams of water.
In the formation of water, if I begin the reaction with 10 grams of H2 and 30 grams of O2, I would expect to form this many grams of water.
33.88 grams water (use 1.88 moles water formed from O2 (the limiting reactant))