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Chemistry > Stoic > Flashcards

Stoic Flashcards

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1
Q

Pure substance

A

matter is anything that takes up space

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2
Q

Elements

A

atoms all having the same numbers of protons

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3
Q

Molecules

A

two or more elements chemically joined together

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4
Q

Compounds

A

Two or more different elements chemically joined together in a fixed ratio

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5
Q

Mixtures

A

a combinations of pure substances

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6
Q

aqueous

A

dissolved in a solvent

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7
Q

physical change

A

no new substances are produced

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8
Q

Chemical change

A

new chemical substance are formed

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9
Q

mole

A

the amount of substances that contains the same number of specified particles as there are atoms in 12g of carbon-12

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10
Q

mole symbol

A

n

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11
Q

avogardos number

A

6.02 x 10 to the power of 23

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12
Q

relative atomic mass

A

the average mass of all isotopes of an element compared to 1/12 the mass of carbon 12 atom

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13
Q

relative formal mass

A

the mass of a molecule compared to 1/12 the mass of C-12 atom

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14
Q

number of moles

A

n = m/M

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15
Q

percentage composition

A

%composition by mass of element = molar mass of x/ molar mass of the compound

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16
Q

Empirical formula

A

the formula of a compounds that shows the lowest whole number ratio of each type of atom

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17
Q

Step to calculate EF

A
  1. Write the elements present in the compound
  2. Write each elements % composition or mass
  3. divide the % or mass by the relative atomic mass and calculate the ratio
  4. divide each ratio by the smallest ratio above to get a whole number ratio
  5. express as empirical formula
18
Q

molecular formula

A

the formula of a compound that shows the actual number of each type of atom in the molecule

19
Q

Atom economy

A

chemical reaction is a measure of the amount of starting material that become useful products

20
Q

calculate atom economy

A

atom economy = total mass of desired products/ total mass of all products or reductants x100

21
Q

Limiting Reactant

A

reactant that will be used up first in a chemical reaction

22
Q

how to determine limiting reactant

A

divide the moles by the leading co-efficient

23
Q

Percentage yield equation

A

percentage yield(%)= actual yield/ theoretical yield x100

24
Q

percentage yield

A

amount of product produced experimentally compared to the theoretical waver.

25
Q

Theory of an ideal gas

A
  • gaseous particles are in continuous random motion, in straight lines not curved.
  • perfect elastic Collison
  • average kinetic energy is directly proportional to temperature
  • volume of gas is negligible
    -no intermolecular forces
26
Q

Ideal gas equation

A

PV=nRT

27
Q

universal gas constant

A

8.31

28
Q

charles law

A

V/T=k

29
Q

boyles law

A

PV=k

30
Q

real gases

A
  • gas particles have volumes
  • particles have attractive forces
31
Q

Ideal Gases

A
  • gas particles do not have volume
  • no attractive forces between particles
32
Q

gas behaviour

A

a gas behaves more ideal at a high temperature and lower pressure
higher temperature: the potential energy due to intermolecular forces become less significant compared with the particles kinetic energy
Low Pressure: the size of molecules become less significant compared to the empty space between them

33
Q

Molar volume

A

the volume occupied by one mole of a substance at a given tempature and pressure

34
Q

STP

A

273K and 100kPa

35
Q

Vm at STP

A

22.7dm3

36
Q

solute

A

the smallest component in a solution

37
Q

solvent

A

the largest component of a solution

38
Q

Solution

A

the solute and solvent combinded

39
Q

Concentration

A

a measure of solute

40
Q

concentration equation

A

concentration = mole of solute/ volume of solution c=n/v

41
Q

dilution

A

the process of adding more solvent to a solution

42
Q

dilution formula

A

C1V1=C2V2

Chemistry (4 decks)

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