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
Can’t 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 + O H2O
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 = O = 16.00
Multiply by number of atoms (if > 1)
Example H x 2 = 2.016
Total these up to determine actual weight of entire molecule
Example H2O = =
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 = kg, lbs, tons
O = x 2 = kg, lbs, tons
* 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 > 0 and < 7)
Sour taste
Vinegar, Hydrocholoric Acid, Hydrofluoric Acid
Base (pH > 7 and < 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