Introduction to Process Technology

1
Introduction to Process Technology

• Unit 5
• Applied Chemistry

2
Agenda

• Organic and Inorganic
• Chemical and Physical Properties
• Terminology
• Reactions
• Chemical Formulas, Calculating Mass
• Acid, Base, pH
• Hydrocarbons
• Other chemical families
• Review

3
Chemistry in Process Industry

• How Chemistry Applies to Process Tech
• Turning raw materials into products
• Proper management of waste
• Understand chemistry concepts that occur during
  manufacturing process
• Understand terminology
• Understand concepts to troubleshoot problems and
  improve quality, efficiency

4
Structure of Matter

• Atoms smallest particle of an element that
  retains the properties of that element
• Protons positively charged subatomic particle
  found in the nucleus of an atom
• Neutrons subatomic particle found in the
  nucleus of an atom that has no charge
• Electrons negatively charged subatomic particle
  found in orbiting the nucleus of an atom
• -- Valence Electrons outermost electrons which
  provide links for bonding

5

• Ions charged particles
• Anion atom or group of atoms with negative
  charge
• Cation - atom or group of atoms with positive
  charge
• Molecule neutral chemically bonded groups of
  atoms that act as a unit
• Isotope element that has same number of protons
  but different number of neutrons

6
Structure of Matter (Continued)

• Atomic Number the number of protons in the
  nucleus of an atom of an element
• Atomic Mass (Molecular Weight) weighted average
  of the masses of the isotopes of an element
  predominantly from masses of protons neutrons
• Determining Molecular Weight
• Add all masses of each element. Remember to
  multiply if more than 1 present.

7
Organic and Inorganic

• Chemistry science that deals with the
  composition, behavior, and transformation of
  matter
• Organic carbon based
• Hydrocarbon contains only hydrogen and carbon
• Inorganic no carbons
• Such as salts, acids, bases, metals
• Many agricultural products

8
Physical Properties

• Density mass (weight) per unit volume
• Specific Gravity comparison of density to that
  of water for solids and liquids and to air for
  gases
• Hardness ability of one substance to
  scratch/mark another
• Odor smell of substance
• Color optical sensation produced by effect of
  light waves stiking surface

9
Reactivity of a Chemical

• The ability of a substance to form new substances
  under given conditions
• A listing of all chemical reactions of a
  substance and the conditions under which the
  reactions can occur

10
Types of Bonds

• Ionic metal and non-metal. Electrons are
  transferred
• Covalent non-metals. Electrons are shared
• Metallic metal to metal. Electrons free flow

11
Terminology

• Matter anything occupying space that has mass
• Element simplest form of matter
• Compound pure substance made up of elements
  that are chemically combined
• Mixture - mixed together, but no chemical
  reaction
• Solution - a homogenous mixture of 2 or more
  substances in a single phase (usually liquid).
  Solute and solvent.

12
Terminology (Continued)

• Solvent substance that dissolves
• Solute substance that is dissolved
• Solubility how well solvent dissolves the
  solute
• Insoluable solute will not dissolve in the
  solvent
• Freezing Point temp. to change liquid to solid
• Melting Point temp. to change solid to liquid

13
Terminology (Continued)

• Boiling Point
• When vapor pressure of liquid equals system
  pressure
• As vapor pressure increases, boiling point
  decreases
• As system pressure increases, so does boiling
  point
• The higher the vapor pressure the more easily a
  material evaporates

14
Terminology (Continued)

• Homogenous
• Same throughout
• Cant tell one part of mixture from another
• Heterogeneous
• Different
• Equilibrium
• Rate of reactants forming products rate of
  products forming reactants

15
Chemical Reactions

• Chemical Reactions
• Endothermic needs/absorbs heat
• Exothermic gives off heat
• Neutralization acid base salt
  water
• Combustion
• fuel oxygen combustion products
  energy light
• Replacement removes minerals from water

16
Chemical Reactions are Affected By

• Heat --- increases molecular activity and
  reaction rate (rates double with each 10)
• Pressure slows molecular movement and changes
  boiling point
• Surface Area solids
• Concentration of liquid and gas components
• Flow Rates of reactants and products

17
Chemical Reactions

• Catalyst
• Helps a reaction start, go at a lower temp, or
  increases rate of reaction
• Is not consumed in the reaction

18
Types of Catalysts

• Adsorption solid that attracts and holds
  reactant molecules so more collisions can occur.
  Also stretches bonds of reactants making them
  easier to break, which requires less energy.

19
Types of Catalysts

• Intermediate attaches to reactant molecules and
  slows it down so collisions can occur
• Inhibitor decreases reaction rate
• Poisoned / Spent no longer functions due to
  contamination or has been used up
• Some can be regenerated

20
Chemical Equations

• Like a recipe
• Must be balanced (same number of atoms of each
  element in reactants as products
• 2H2 O2 2H2O
• reactants products

21
Mass Relationships

• Allows us to take a balanced equation and use it
  to determine the actual mass/weight needed for
  reactants and how much product can be produced

22
Mass Relationships - Steps

• Find molecular weight of each element on periodic
  table (AMUs, but represent grams, pounds, etc.)
• Example H 1.008 O 16.00
• Multiply by number of atoms (if gt 1)
• Example H x 2 2.016
• Total these up to determine actual weight of
  entire molecule
• Example H2O 2.016 16.00 18.016
• Note how reactant mass product mass

23
Mass Relationships - Steps

• Determine how many moles (amounts) of a reactant
  are needed to produce a set amount of product
• Example N2 2O2 ? 2NO2
• So you need 1 mole of N2 and 2 moles of O2 to
  make 2 moles of NO2

24
Mass Relationships - Steps

• Determine the relative volume of reactant or
  product you have
• Example if you only have 16 pounds of O, you only
  have 0.25 volume (16/64)
• Multiply the relative volume by the amount of
  product you can make
• Example 0.25 x 2NO2 0.5 volume of NO2

25
Mass Relationships - Steps

• Multiple the volume you can make by the molecular
  weight of material
• Example 0.5 volume x 46 23 kg, lbs, tons
• N 14.00 kg, lbs, tons
• O 16.00 x 2 32.00 kg, lbs, tons
• 46.00 kg, lbs, tons

26
Material Balances

• Method used to determine the exact amount of
  reactants needed to produce the specified
  products in the quantity desired
• Steps
• Determine the weight of each molecule
• Ensure reactant total weight equals product total
  weight
• Determine relative number of reactant atoms or
  ions

27
Percent by Weight Solutions

• Weight of solute (material that is dissolved) is
  taken in relationship to entire solution
• 650 pound barrel has 10 catalyst solution
• 650 lb x 0.10 (percent as decimal) 65 lbs

28
Acid, Base and pH

• pH measurement of hydrogen ions in solution
• Acid (pH gt 0 and lt 7)
• Sour taste
• Vinegar, Hydrocholoric Acid, Hydrofluoric Acid
• Base (pH gt 7 and lt 14)
• Bitter taste, slippery
• Alkaline
• Caustic pungent odors
• Lye, sodium hydroxide, caustic soda
• Neutral pH 7
• The stronger the acid or base the more hazardous
  to body tissue and metal

29
Hydrocarbons

• Compound that contains both hydrogen and carbon
• Fossil fuels oil natural gas, and their
  refined products (gasoline, ethylene)

30
Hydrocarbons

• Major groups
• Alkanes single covalent bond (methane, propane,
  ethane, etc)
• Olefins not naturally occurring. Produced by
  cracking oil or natural gas. At least one double
  bond (hence the high energy when used)
• Alkenes double bonds (ethylene, propylene)
• Alkyne triple bonds (acetylene only one used
  widely)
• Cycloalkane contains a ring or cycle of carbons
• Aromatic contains at least one highly
  unsaturated six-carbon ring

31
Aromatic Hydrocarbons

• Include both hydrocarbons and compounds that
  cannot be classified as hydrocarbons
• Most common - benzene

32
Alcohols

• Compounds that contain OH goups connected to an
  alkyl carbon.
• Ethanol commonly referred to as grain alcohol
  since often produced from corn, rye, wheat,
  molasses (from sugar cane), grapes and potatoes.
  
• Becoming popular as gasoline additive or main
  fuel.

33
Alcohols

• Methanol referred to as wood alcohol, because
  it was originally derived from wood.
• Now produced by subjecting H to CO3 at high temp.
  in presence of catalyst.
• Used as solvent in paints, varnishes, production
  of formaldehyde, cleaners.

34
Alcohols

• Isopropyl Alcohol most common is rubbing
  alcohol used externally for cooling skin,
  disinfect cuts, cosmetic solvent

35
Phenols

• Similar to alcohols, but have an OH group
  connected directly to an aromatic ring.
• Used in antiseptics, dyes, aspirin, and at one
  time throat lozenges

36
Ethylene Glycol

• Highly reactive ethylene oxide is reacted with
  water
• Commonly used as antifreeze in vehicle radiators
  because of unique abiltiy to lower freezing point
  of water.
• Also has higher boiling point than water so
  better suited to high and low temp. variations
  due weather extremes.
• Because of toxicity when ingested there is a move
  to switch to less toxic propylene glycol which
  many countries in Europe have already done

37
Applied Concepts

• Distillation separation of various fractions in
  a mixture by individual boiling points
• Reactors designed to break or make chemical
  bonds which changes reactants into products

38
Applied Concepts

• Catalytic Cracking splits side stream of
  fractionating column into smaller, more useful
  molecules for example, kerosene into hexane and
  hexene
• Hydrocracking process used to boost gasoline
  yield
• Alkylation uses a reactor to make one large
  molecule out of smaller ones. For example
  isobutane and olefins into high octane alkylates

39
Review

• List importance of applied chemistry to process
  technicians
• Re-write all vocabulary words and their
  definitions
• Understand difference between the following
• Organic and inorganic
• Endothermic and exothermic
• Acids and bases
• Define the 4 basic chemical reactions most common
  to process industry

40
Work

• Read CAPT Chapter 11 (pages 158 169)
• Do questions 1 13 on pages 170 171)
• Read Thomas Chapter 13 (pages 281 302
• Do questions 1 21 on page 303
• Module 5, Exercise 1 Chemistry Supplement
• Major Grade
• In class example worked by group

41
Independent Project

• Internet or literature search
• Write a paper on the importance of chemistry to 2
  different process industries
• List raw materials, products
• List what chemical reactions, terms apply
• Identify associated safety and environmental
  measures and/or concerns