quantitative chem 3 Flashcards

1
Q

percentage mass of an element in a compound =

A

Ar * number of atoms of that element/

Mr of the compound * 100

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2
Q

moles =

A

mass / Mr

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3
Q

volume of gas =

A

mass of gas /

Mr of gas *24

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4
Q

concentration (g/dm cubed) =

A

mass(g) /

volume (dm cubed)

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5
Q

concentration(mol/dm cubed) =

A

number of moles(mol) /

volume (dm cubed)

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6
Q

atom economy =

A

relative formula mass of desired products /

relative formula mass of all reactants *100

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7
Q

percentage yield =

A

mass of product actually made /

maximum theoretical mass of product *100

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8
Q

Why do you never get 100% yield

A

Not all reactants react to make a product(reversible)
There might be side reactions
You lose some product when you separate it from the reaction mixture

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9
Q

(yield) what happens if you want to keep the liquid

A

you lose a bit that remains with the solid and filter paper

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10
Q

(yield) what happens if you want to keep the solid

A

some of it will get left behind when you scrape it off the paper

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11
Q

what is the atom economy

A

tells you how much of the mass of the reactant is wasted when manufacturing a chemical and how much ends up as useful product

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12
Q

disadvantages of low atom economy

A
use up resources quickely
make lots of waste product
unsustainable
aren't profitable
raw materials are expensive
waste is expensive to remove
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13
Q

the best way of getting rid of waste product

A

find a use for it

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14
Q

what is concentration

A

The amount of a substance in a certain volume of a solution

The more solute the more concentrated

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15
Q

why is the a amount of product formed directly proportional to the amount of limiting reactant

A

if you add more reactant there will be more reactant particles to take part in the reaction.

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16
Q

step to find the limiting reactant

A

1) Write out balanced equation
2) work out Mr
3) find out the moles there are of the known substance
4) use the balanced equation to work out the moles needed of the other
5) calculate mass

17
Q

steps to balance equations using reactant masses

A

1) divide the mass of each substance by it’s Mr to find the moles
2) Divide the moles by the smallest number of moles in the reaction
3) make sure they are all whole numbers
4) re write the balanced equation

18
Q

what is one mole of a substance

A

is just an amount of that substance that contains an Avogadro number of particles- 6.02 * 10 to 23 particles`

19
Q

What happens to the number of atoms during a reaction

A

no atoms are destroyed and no atoms created this means that the same number of atoms are on each side so are conserved

20
Q

How to find out if the mass is conserved

A

1)add up the the relative formula masses of the substance on each side

21
Q

explanation 1 of why mass seems to change(reactant is gas)

A

one of the reactants is a gas and all the products are solids, liquids.

Before the reaction the gas is floating in the air

when the gas reacts to form a product it becomes contained so the total mass of the stuff in the reaction increases.

22
Q

explanation 2 of why mass seems to change(product is gas)

A

product is gas and all reactants are solids

Before the reaction all the reactants are contained

If the vessel isn’t enclosed then the gas can escape from the reaction