Chapter 3 - Amount of Substance Flashcards

1
Q

How many particles in a mole?

A

6.02 x 10^23 (Avogadro constant)
This is the number of particles in 12g of Carbon-12

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2
Q

What is molar mass?

A

Molar mass gives the mass in grams in each mole of the substance

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3
Q

What is the equation for moles?

A

moles (mol) = mass (g) / Molar mass (g/mol)

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4
Q

What is an empirical formulae?

A

It is the simplest whole-number ratio of atoms in a compound.

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5
Q

What is the equation for moles of gas at RTP?

A

At 298K and 100kPa
moles (mol) = volume of gas (dm^3) / 24 dm^3

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6
Q

What is the ideal gas equation?

A

pV = nRT
p = pressure (Pa)
V = volume (m^3)
n = moles (mol)
R = ideal gas constant (8.314 J mol^-1 K^-1)
T = temperature (K)

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7
Q

Convert cm^3 to m^3

A

x 10^-6

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8
Q

Convert dm^3 to m^3

A

x 10^-3

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9
Q

Convert degrees C to K

A

+273

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10
Q

Convert kPa to Pa

A

x 10^3

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11
Q

Convert 1atm to kPa and Pa

A

100 kPa or 100000 Pa

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12
Q

What is the molecular formula?

A

The number of atoms of each element in a specific molecule.
e.g. O2

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13
Q

What does anhydrous mean?

A

A substance that does not contain water that is often crystalised

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14
Q

What does hydrated mean?

A

A compound that contains water molecules and is part of the crystalline structure.

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15
Q

What is a limiting reagent?

A

A product that is not in excess so will be completely used up first and stop the reaction.

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16
Q

Why is it important for reactions to have high atom economy?

A

More sustainable
Means that toxic/unwanted products aren’t released that could be potentially toxic to the environment
Also excess energy isn’t used to produce unwanted products