C5 Seperate chemistry 1 Flashcards

1
Q

How do you calculate concentration?

A

conc = moles dissolved/ vol of solution

mol
dm^3

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2
Q

How do you convert g/dm^3 into mol/dm^3 ?

A

divide by relative formula mass

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3
Q

How do you convert mol/dm^3 into g/dm^3 ?

A

multiply by relative formula mass

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4
Q

How do you calculate percentage yield?

A

% yield = (actual yield/ theoretical yield) x100

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5
Q

What is the actual yield in comparison to the theoretical yield?

A

less than

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6
Q

What causes the actual yield to be less than the theoretical yield?

A
  • incomplete reactions
  • impure reactants
  • practical losses during the experiment
  • unwanted side reactions
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7
Q

What is atom economy?

A

% of mass of reactants that ends up being the desired product

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8
Q

How do you calculate atom economy?

A

(mr of desired products/ mr of all products) x100

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9
Q

What factors affect the reaction pathway of a specific product and why?

A

atom economy
-want a reaction with least waste products

yield
-want to produce as much as possible

rate
-want to make the most at fastest speed

usefulness of by-products
-want to reduce waste

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10
Q

What is the molar volume of any gas at room temperature + pressure?

A

volume occupied by one mole of molecule of any gas at room temperature+pressure

volume = molar vol x moles

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11
Q

How do you calculate molar volume?

A

mol vol = gas vol/ no. moles

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12
Q

How can we calculate gas vol from a balanced equation?

A

1
identify product and reactant in question

2
work out no. moles of reactant

3
use the balanced equation to work out the ratio of moles between the reactant and the product

4
use ratio to work out the no. moles of the product

5
use avogadros law to work out volume of product

avogadros law:
volume = mol vol (usually 24dm3) x number of moles

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13
Q

How can we use the volume of one gas to find the volume of another?

A

1
ratio the coefficient of the rectant with known volume with the product in question

2
use volume to find the volume of the product

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14
Q

What is the harber process?

A
  • reversible reaction

- nitrogen + hydrogen <=> ammonia

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15
Q

How is the rate of attainment of equilibrium affected by changes in temperature?

A
  • if temperature is increased
  • dynamic equilibrium opposes this change
  • by decreasing the temperature
  • favours endothermic reaction
  • lower temperatures mean slower RoR
  • takes longer to produce same % yield of product
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16
Q

How is the rate of attainment of equilibrium affected by changes in pressure?

A
  • if pressure is increased
  • dynamic equilibrium opposes this change
  • it will do this by decreasing the number of molecules in the reaction
  • increasing pressure means stronger, more expensive equipment is needed
  • increases cost
17
Q

How is the rate of attainment of equilibrium affected by changes in concentration?

A
  • if more reactant is added
  • dynamic equilibrium opposes this change
  • by decreasing amount of reactant in reaction
18
Q

How is the rate of attainment of equilibrium affected by the use of a catalyst?

A
  • increases RoR

- temperatures dont need to be high to maximise % yield

19
Q

What may fertilisers contain?

A
  • nitrogen
  • phosphorus
  • potassium
20
Q

How are fertilisers formed from ammonia and why?

A

ammonia + nitric acid -> ammonium nitrate

ammonium nitrate
-NH4NO
–has a high proportion of nitrogen per unit mass
–nitrogen good for plant growth

21
Q

How is ammonium sulphate produced by laboratory production?

A

ammonia solution + dilute sulfuric acid

stage one
-pipette 25cm3 of ammonia solution in conical flask

stage two
-titration

stage three
-mix same volumes of ammonia and sulfuric acid determined in the titration with no indicator

stage four
-preparation of pure, dry crystals of ammonium sulfate

22
Q

How is ammonium sulphate produced by industrial production?

A
  • lots of stages needed
  • ammonia and sulfuric acid have to be made from raw material first
  • use a large reaction chamber filled with ammonia gas
  • sulfuric acid is sprayed into chamber where it reacts with the ammonia
  • to produce ammonium sulphate
23
Q

Describe the titration of ammonia solution with dilute sulfuric acid (ammonia solution in conical flask)

A
  • add a few drops of methyl orange to the ammonia solution
  • fill a burette with sulfuric acid.
  • read the level of the burette
  • add acid from the burette swirling gently
  • add drop-by-drop near the end-point until the indicator just changes colour
  • read the level in the burette and record the volume of acid used
  • repeat until results are concordant
24
Q

Describe the steps of preparing pure, dry crystals of ammonium sulphate ( solution already prepared)

A
  • pour solution into an evaporating dish and heat to dryness
  • until pure crystals form
  • leave to cool
  • filter off crystals
  • wash with distilled water
  • leave to dry
25
Q

Why isn’t laboratory production of ammonium sulfate suitable for industrial use?

A
  • volumes required are too large to titrate
  • volumes of solutions are too large to be heated for evaporation
  • crystallisation process is too slow