The Mole. Chapter 11. Particles Names. Atoms, formula units (ionic compounds), molecules (covalent compounds). Counting units. 1mole = 6.02 x 10 23 particles. Mole to Particle Conversions. How many molecules of water are there in 2.4 moles of water?
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How many molecules of water are there in 2.4 moles of water?
How many moles of copper contain 3.5 x 1018 copper atoms?
According to Avogadro, the mass of one mole of a gas at STP is always 22.4L regardless of the gas’ identity.
STP = Standard Temperature and Pressure (0oC and 1 atmosphere)
The mass of one mole of a substance is unique to that substance and is based on the sum of the atomic masses of the elements in that substance.
1 mole of copper = 63.6g
1 mole of lead = 207.2g
1 mole of water = 18.0g
Mass of H2O = mass of two hydrogen atoms + mass of one oxygen atom
Sum of the product of the number of each atom and their masses divided by the total mass of the compound
What is the percent composition of Mg(BrO4)2?
1(mass Mg) + 2(mass of Br) + 8(mass of oxygen) = Mass of Mg(BrO4)2
Chemical formula which contains the lowest whole number ratio of atoms
Ionic formulas always contain the lowest whole number ratios
Covalent compounds do not always contain the lowest whole number ratios
What is the Empirical Formula of the following compounds?
What is the empirical formula for a compound which contains 25.9% nitrogen and 74.1% oxygen by mass?
Assume a 100g sample. In that sample 25.9 g is nitrogen and 74.1g is oxygen
What is the molecular formula of a compound with an empirical formula of CH2O and a molecular mass of 90g/mol?
CH2O =1(12g)+2(1g)+1(16g) = 30g
Determine the molecular formula of a compound that has a mass of 34g and contains 94.1% oxygen and 5.9% hydrogen by mass.