Quantitative chemistry Flashcards

1
Q

It is not always possible to obtain a calculated amount of products because:

A
  • the reaction may not go to completion since it is reversible
  • some of the product may be lost when it is separated from the reaction mixture
  • some of the reactants may react in different way than expected
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2
Q

Relative formula mass of a molecule is also known…

A

as relative molecular mass.

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3
Q

Relative atomic mass

A

The average mass of the isotopes of the element weighted to take into account the abundance of each isotope. This is then compared with carbon-12 (6 protons and 6 neutrons).

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4
Q

A formula for relative atomic mass

A

Ar=( mass number of isotope 1 x percent abundance of isotope 1 )+(mass number of isotope 2 x percent abundance of isotope 2) / 100

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5
Q

The Mole

A

The relative atomic mass of any substance expressed in grams.

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6
Q

Relative formula mass of a compound…

A

is the sum of the relative atomic masses of the atoms in the numbers shown in the formula. Mr

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7
Q

Relative atomic mass is…

A

a mass number of elements. Ar

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8
Q

Abundance

A

How common it is.

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9
Q

One mole contains

A

6.02 x 10 (to the power of 23) atoms or molecules.

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10
Q

The mole number is known as…

A

Avogadro’s number.

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11
Q

Relative formula mass has…

A
  • no units

- never involves big numbers

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12
Q

A formula for moles of an element

A

num of moles = mass (g) / relative atomic mass (Ar)

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13
Q

A formula for moles of a compound

A

num of moles = mass(g) / relative formula mass (Mr)

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14
Q

Empirical formula

A

The simplest ratio of each type of atom in the compound. It must be a whole number.

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15
Q

The concentration of a solution is related to…

A

the mass of the solute (moles) and the volume of the solution.

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16
Q

Concentration formula

A

c (mol/dm3) = number of moles / volume of solution (dm3)

17
Q

The Ar of any element is equal…

A

to one mole.