MR Chard Flashcards

0
Q

define relative molecular mass (Mr)

A

the average mass of a molecule compared to 1/12 th the mss of an atom of carbon 12

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1
Q

Define Relative atomic mass (Ar)

A

the average mass of an atom compared to 1/12 th the mass of carbon 12

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2
Q

define the MOLE

A

one mole of a substance is the amount of that substance which contains as many entities as there are in exactly 12g of carbon 12

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3
Q

Equation for moles, mass and mr

A

N= m/mr

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4
Q

Ideal gas equation

A

pV=nRT

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5
Q

pV=nRT

What does p stands for? And what unit is it measured in?

A
Pressure
Pascals (1pa=1N per meter squared )
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6
Q

pV=nRT

What does the v stand for and what unit is it measured in?

A

Volume

Meters squared

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7
Q

pV=nRT

What does the n stand for and what unit is it measured in?

A

Mols

Mols

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8
Q

pV=nRT

What dies the R stand for and what unit is it measured in?

A

Gas constant

8.31 J Km-1 mol-1

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9
Q

pV=nRT

What does the T stand for and what unit is it measured in?

A

Temperature

Kelvin- 0’= 273K

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10
Q

M(cubed)to dm(cubed)

A

X1000

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11
Q

Dm(cubed) to m(cubed)

A

/ 1000

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12
Q

Cm(cubed) to m(cubed)

A

/ 1,000,000

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13
Q

M(cubed) to cm(cubed)

A

X1,000,000

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14
Q

Pressure- Kilo Pascals to Pascals

A

100kpa = 100,000pa (x1000)

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15
Q

equation for concentration

A

n= cxv
____
1000

16
Q

what is concentration?

A

distance of particles from one another

17
Q

alternate equations for n= cxv
____
1000

A

c= nx1000
_______
v

v= nx1000
______
c

18
Q

atom economy equation

A

% atom economy= (mass of desired product / mass of all reactants)x100

19
Q

in atom economy, one product =

A

100% atom economy

20
Q

how do you work out apparatus error

A

error
______ x100
total

e.g. 0.001
_______ x100 =0.4%
2.53