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Chemistry 1A > Week Six > Flashcards

Week Six Flashcards

1
Q

Gases

A

expand to occupy all the space
free to move
very weak forces

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2
Q

Boyles Law

A

volume is inversely proportional to the total pressure

P1V1=P2V2

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3
Q

Charles Law

A

volume is directly proportional to temp

V1/T1 = V2/T2

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4
Q

Avogadros law

A

gas volume is proportional to the amount of gas

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5
Q

ideal gas equation

A

PV = nRT

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6
Q

R

A

8.314

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7
Q

Pressure, Volume moles and temp equation

A

P1V1/N1T1 = P2V2/N2T2

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8
Q

Kinetic energy

A

1/2mu^2`

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9
Q

Average kinetic energy

A

3RT/2Na
t = temp
Na = avogardos constant
R = gas constant

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10
Q

Total amount of gas

A

n(molecule 1) + n(molecule 2)

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11
Q

Gas Density

A

pM/Rt

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12
Q

Dispersion forces

A

are the attractions between the negatively charged electron cloud of one molecule and the positively charged nuclei of neighbouring molecules

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13
Q

Dipole induced dipole forces

A

stornger than dispersion forces

molecule with permenant dipole induces a dipole in neighbouring molecule

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14
Q

dipole dipole forces

A

attractions between negatively charged end of polar molecules and the positviely charged end of neighbouring polar molecule

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15
Q

reactive metal + acid

A

hydrogen gas and metal salt

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16
Q

net ionic equation

A

only shows the ions which are in reaction not including spectator ions

17
Q

redox reaction

A

oxidation/ reduction reaction

18
Q

half equations

A

individual equations of the oxidised and reduced parts

19
Q

Reducing agent

A

species that reduces the other, is being oxidised

20
Q

Oxidising agent

A

oxidises the other species, is reduced

21
Q

The activity series

A

ease of oxidation increases up the table

22
Q

1 pascal

23
Q

standard atmospheric pressure

24
Q

Gay Lussac law

A

pressure is directly proportional to temp

p1/T1 = P2/T2

25
Q

Daltons law of partial pressure

A

for unpure gases

26
Q

Ptotal

27
Q

Ptotal equation

A

RT/V (n1+n2)

28
Q

X1

A

(n1RT/v)/ (n1+n2)RT/V

29
Q

using X1 to get total

A

P1 = X1 x Ptotal

30
Q

Kinetic theory of Gases

A

physical properties of gases can be explained in terms of motion of indivual particles

31
Q

deviation from ideal behaviour

A

when pressure is increased or gas is cooled intermolecular forces become significant enough to affect the motion of the molecules and gas wont behave ideally

32
Q

Van der waals equation

A

van der waals equation slightly lowers the gas pressure

33
Q

pideal = preal + an2/V2

A 
a = constant 
n = moles
v = volume
34
Q

R constant in Atm, L, mol and K

35
Q

R constant in Pa, m3, mol, and K

36
Q

Unknown Molar mass

Chemistry 1A (12 decks)

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