Chemistry 1.2: Amounts Of Substance Part 1
This flashcard set explains key terms in chemical calculations, including relative atomic, molecular, and formula masses. It also defines the mole and Avogadro’s constant, fundamental concepts for understanding the quantitative aspects of chemistry.
Relative atomic mass
Weighted average mass of all the isotopes relative to 1/12th mass of an atom of carbon-12
Key Terms
Relative atomic mass
Weighted average mass of all the isotopes relative to 1/12th mass of an atom of carbon-12
Relative molecular mass
Mass of a molecule of the compound relative to 1/12th of the mass of an atom of carbon-12
Relative formula mass
Mass of one formula unit of an ionic compound relative to 1/12th mass of an atom of carbon-12
Mole
Amount of substance that contains as many particles as there are in exactly 12g of carbon-12
Avogadros constant
02x10 (to the power) 23
or. There are 6.02x10 (to the power) 23 atoms of carbon in 12g c...
Does a mole of one substance contain the same number of particles as a mole of any other substance
Yes
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| Term | Definition |
|---|---|
Relative atomic mass | Weighted average mass of all the isotopes relative to 1/12th mass of an atom of carbon-12 |
Relative molecular mass | Mass of a molecule of the compound relative to 1/12th of the mass of an atom of carbon-12 |
Relative formula mass | Mass of one formula unit of an ionic compound relative to 1/12th mass of an atom of carbon-12 |
Mole | Amount of substance that contains as many particles as there are in exactly 12g of carbon-12 |
Avogadros constant |
or. There are 6.02x10 (to the power) 23 atoms of carbon in 12g carbon-12 |
Does a mole of one substance contain the same number of particles as a mole of any other substance | Yes |
What do you need to know to calculate moles in a solid | Mass |
What do you need to calculate the number of moles in a gas | Volume |
What do you need to know to calculate the number of moles in a solution | Volume and concentration |
How do you get from Mg to mg | /1000 |
How to you get from mg to g | /1000 |
How do you get from Mg to g | /1000000 |
How to get from g to kg | /1000 |
How to get from kg to tonnes | /1000 |
How to get from g to tonnes | /1000000 |
How to get from tonnes to kg | X1000 |
How to get from kg to g | X1000 |
How to get from tonnes to g | X1000000 |
How to get from g to mg | X1000 |
How to get from g to Mg | X1000 |
How to get from g to Mg | X1000000 |
Formula for calculating moles in solids | Mass (in g) = moles x Mr |
How to calculate the number of atoms in a gives mass | First calculate number of moles using mass/Mr Then calculate number of atoms using moles x avogadros constant |
How to get from centimetres cubed to decimetres cubed | /1000 |
What do you need to know in order to calculate the number of moles in a solution | Volume in demimetres cubed | Concentration in moles per decimetres cubed |
What is concentration | The number of moles of a solute dissolved in one decimetre cubed of solution |
What is the formula to work out the number of moles in a solution | Moles = volume x concentration |
How to calculate the concentration of a solution given the mass and volume | |
What are the assumptions made when using the ideal gas equation to |
| * the volume occupied by the molecules is entirely negligible relative to the volume of the container |
What is the ideal gas equation | pV = nRT |
What unit is the answer always given in | Metres cubed |
What is pressure measured in | Pascals, Pa |
How to get from kPa to Pa | X 1000 |
How to get from MPa to Pa | X1000000 |
What is volume measured in | Metres cubed |
How to get from centimetres cubed to metres cubed | /1000000 |
How to get from decimetres cubed to metres cubed | /1000 |
What is n | Number of moles |
What is R | Gas constant: 8.314 |
What is T measured in | Kelvin, K |
How to get from Celsius to kelvin |
|
How to get from kelvin to Celsius | -273 |
What is density | It's mass per unit volume |
Formula for density | Mass = density x volume |
What is density usually measured in | Grams per centimetre cubed |
Empirical formula | Simplest whole number ratio of atoms of each element present in a molecule |
Molecular formula | Actual number of atoms of each element present in a molecule |
How to calculate molecular formula | Calculate empirical formula |