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Chemistry > Unit 3 - Chemistry in Society > Flashcards

Unit 3 - Chemistry in Society Flashcards

1
Q

Simple distillation steps

A
  1. Place the liquid and dissolved solid into the flask
  2. Evaporate the liquid by heating
  3. Use a thermometer blocking the top of the tube to monitor the temperature
  4. Direct the vapour down a side pipe with a condenser
  5. Use running tap water flowing through the condenser
  6. Collect the condensed liquid in a beaker
  7. Left with solid crystals in the flask and liquid in the beaker
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2
Q

Factors influencing sustainable industrial process design

A
  • availability
  • sustainability
  • cost
  • opportunities for recycling
  • energy requirements
  • marketability of biproducts
  • product yeild
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3
Q

Environment considerations for industrial process design

A
  • minimizing waste
  • avoiding toxic substances
  • biodegradable products
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4
Q

Feedstock availability sustainability and cost profit gain and loss

A

Gain - local availability

Loss - scarcity, transport- safety, cost, environmental

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5
Q

Opportunities for recycling in industrial processes profit gain and loss

A

Gain - efficiency^, reduce waste

Loss - difficulty separating unreacted stuff makes it inefficient

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6
Q

Energy requirements and Industrial processes profits gain and loss

A

Gain - exothermic reactions to keep heat in reaction, or even building; catalysts

Loss - reactions needing heat or cooling can be expensive

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7
Q

Use of byproducts in industrial processes profits gain and loss

A

Gain - selling biproducts or using elsewhere in a process

Loss - toxic biproducts difficult

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8
Q

Product yield in industrial processes profit gain and loss

A

Gain - high yield is profitable

Loss - low yields need more expensive repetition of reaction

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9
Q

For n=cV volume must be in

A

LITRES

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10
Q

Mv

A

V/m

Volume per mole

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11
Q

Relative rate equation

A

Rate = 1/time

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12
Q

Time from relative rate

A

Time = 1/relative rate

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13
Q

Collision theory requirements for a reaction

A
  • correct collision geometry
  • sufficient energy to reach an activated complex
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14
Q

Effects on rate

A
  • concentration/ pressure
  • particle size
  • temperature
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15
Q

Energy distribution diagram for lower energy complex

A

Y axis = no. of molecules
X axis = kinetic energy

Steeper rising limb, peaks sooner and higher, smaller section past the E(A) line

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16
Q

Energy distribution diagram for higher energy complex

A

Y axis = no. of molecules
X axis = kinetic energy

More gentle rising limb, peaks later, greater section past the E(A) line

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17
Q

Temperature is

A

The measure of the average kinetic energy of the particles in a substance

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18
Q

The activation energy is

A

The minimum kinetic energy required by colliding particles before a reaction may occur

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19
Q

Changing concentration, pressure or particle size impacts the reaction rate because

A

The number of collisions are increased

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20
Q

Change in temperature effects the reaction rate because

A

Reacting particles have sufficient energy

21
Q

In an exothermic reaction the products have ____ energy than the reactants because

A

Less, energy is being released to the surroundings

22
Q

In the endothermic reaction the enthalpy change is ______ because

A

Positive, the reactantion gains energy from its surroundings

23
Q

ΔH =

A

H(products) - H(reactants)

24
Q

The activated complex is

A

A high energy, unstable arrangement of atoms

25
Q

Increasing temperature does not affect the activation energy, whereas ______ do

A

Catalysts

26
Q

The enthalpy of combustion is

A

The enthalpy change when one mole of a substance is burned completely in oxygen

27
Q

Apparatus to measure the enthalpy of combustion

A

Copper can, thermometer, water, all above the combusting fuel and surrounded by draft shield

28
Q

The enthalpy of combustion will always be

A

Negative, and in kJ mol¯¹

29
Q

When using cm³ water measurements in enthalpy change calculations

A

Remember to convert to kilograms

30
Q

Hess’s law

A

The enthalpy change of a chemical reaction is independent of the route taken

31
Q

When calculating Bond enthalpies, remember breaking bonds

A

Requires energy

32
Q

When calculating Bond enthalpies remember

A

Making bonds releases energy

33
Q

Molar bond enthalpy is

A

The energy requires to break one mole of bonds in a diatomic molecule

34
Q

Equilibrium is where

A

The rate of the forward reaction equals the rate of the backwards reaction

35
Q
A
35
Q

Concentrations of reactants and products at equilibrium are _______ but rarely _______

A

Constant, equal

36
Q

How do catalysts impact equilibrium

A

They don’t move the equilibrium but may increase the speed at which it is reached

37
Q

Effect of addition of an alkali on equilibrium when the product includes H+ ions

A

Right, as the the alkali removes H+ ions and the forwards reaction will replace them

38
Q

If you increase pressure the equilibrium will shift to____

A

Get rid of whichever side has more mols of gas

39
Q

If the forward reaction is exothermic then an increase in temperature will..

A

Favour the backwards reaction, equilibrium shifts left

40
Q

Chromatography is used to

A

Separate components within a mixture

41
Q

Effects on chromatography results

A
  1. Polarity - solubility in p/np solvent
  2. Molecular size
42
Q

Type of chromatography results

A

Distance or time against response graph

43
Q

Concordant titre volumes

A

0.2cm³

44
Q

Titration not requiring an indicator

A

Acidified permanganate, since it already goes purple to colourless

45
Q

Titration is used to determine

A

The volume of a solution required to reach the end point of a reaction

46
Q

Phenolphlaline colour change

A

Adic - colourless
Basic - pink

47
Q

Standard solutions

A

Solutions of accurately known concentration

Chemistry (6 decks)

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