Environmental Chemistry I

Code:

EA0007

Acronym:

QA I

Keywords
Classification	Keyword
OFICIAL	Basic Sciences
OFICIAL	Design, Development, Implementation and Operation
OFICIAL	Interp/Personal professional attitudes and capac.

Instance: 2009/2010 - 1S

Active?	Yes
Responsible unit:	Department of Chemical and Biological Engineering
Course/CS Responsible:	Master in Environmental Engineering

Cycles of Study/Courses

Acronym	No. of Students	Study Plan	Curricular Years	Credits UCN	Credits ECTS	Contact hours	Total Time
MIEA	58	Syllabus since 2006/07	1	-	6,5	56	175

Teaching language

Portuguese

Objectives

1. Background
Using the principles of chemistry, environmental engineers develop ways to solve problems related to the environment. They are playing their part in the big environmental issues such as air and water pollution control, waste disposal, recycling, ozone depletion, global warming and the like. Many of these issues involve understanding chemical reactions.
2. Specific aims
This basic course intends (i) to pass on fundamental knowledge of chemistry that will support the student’s education regarding environmental chemistry and (ii) to give a global vision of fundamental chemistry in an interface framework with environment and environmental chemistry;
3. Previous knowledge:
Basic knowledge of chemistry.
4. Percent distribution:
Scientific component: 100%
Technological component: 0%
5. Learning outcomes
It is expected that students have:
- deepen and consolidated their previous acquired knowledge on chemistry;
- developed a scientific reasoning and a critical mind, avoiding the primary acceptance of results;
- increased their auto-sufficiency by valuing the search and use of recently published data.

Program

1. Revision of basic concepts
1.1 Elements e atoms
1.2 Compounds
1.3 Nomenclature of inorganic compounds
1.4 Unities and measurements
1.5 Moles e molar weights
1.6 Determination of chemical formulas
1.7 Mixtures and solutions
1.8 Chemical equations
1.9 Aqueous solutions (concentration and dilution)
2 The Properties of Gases
2.1 The nature of gases
2.1.1 Pressure and its unities
2.2 The gas laws
2.2.1 Boyle’s law
2.2.2 Charles’s law
2.2.3 Avogadro’s principle
2.2.4 The ideal gas law
2.2.5 Gas density
2.2.6 The stoichiometry of gaseous reactions
2.2.7 Mixtures of gases
2.3 Real gases
2.3.1 Deviations from ideality
2.3.2 The liquefaction of gases
2.3.3 Equation of state of real gases
2.4 Chemistry in the atmosphere
2.4.1 Earth's atmosphere. Phenomena in the outer layers of the atmosphere.
2.4.2 Depletion of ozone in the stratosphere
2.4.3 The greenhouse effect.
2.4.5 Photochemical smog.
3 The Properties of Liquids
3.1 Intermolecular forces
3.1.1 The formation of condensed phases
3.1.2 Ion-dipole forces
3.1.3 Dipole-dipole forces
3.1.4 London forces
3.1.5 Hydrogen bonding
3.2 Liquid structure
3.2.1 Order in liquids
3.2.2 Viscosity and surface tension
3.2.3 Water. Structure and properties.
4 Termochemistry
4.1 Systems states and energies
4.1.1 Systems
4.1.2 Energy and work
4.1.3 Heat
4.1.4 The first law of thermodynamics
4.1.5 State functions
4.2 Enthalpy
4.2.1 Heat capacities of gases
4.2.2 Enthalpy of phase changes
4.2.3 Heating curves
4.2.4 Reaction enthalpies
4.2.5 The relation between enthalpy and internal energy
4.2.6 Standard reaction enthalpies
4.2.7 Hess’s law
4.2.8 The heat output of reactions
4.2.9 Influence of temperature on the reaction enthalpy
5 Spontaneous and Non-Spontaneous Changes
5.1 Entropy
5.1.1 Spontaneous change
5.1.2 Entropy and disorder
5.1.3 Entropy changes accompanying changes of physical state
5.1.4 Standard molar entropies
5.1.5 Standard reaction entropies
5.2 Global changes in entropy
5.2.1 The surroundings
5.2.2 The overall change in entropy
5.2.3 Equilibrium
5.3 Gibbs energy
5.3.1 Reaction Gibbs energy
5.3.2 The effect of temperature on the change of Gibbs energy
5.3.3 Change of Gibbs energy and equilibrium
6. Physical equilibria
6.1 Phases and phases transitions.
6.1.1 Vapor pressure. The variation of vapor pressure with temperature.
6.1.2 Boiling. Freezing and melting.
6.1.3 Phase diagrams. Critical properties.
6.2 Solubility
6.2.1 The like- dissolves -like rule.
6.2.2 Pressure and gas solubility: Henry's law.
6.2.3 Temperature and solubility.
6.2.4 The enthalpy of solution.
6.2.5 The free energy of solution.
6.3 Colligative properties
6.3.1 Vapor-pressure lowering
6.3.2 Boiling-point elevation and freezing-point depression
6.3.3 Osmosis.
6.4 Binary liquid mixtures
6.4.1 The vapor pressure of binaryliquid mixtures.
6.4.2 Distillation.
6.4.3 Azeotropes.
7. Concepts of organic chemistry
7.1 Common functional groups. Nomenclature of organic compounds.
7.2 Aliphatic hydrocarbons. Physical and chemical properties.
7.3 Aromatic hydrocarbons.Physical and chemical properties.
7.4 Properties and reactions of compounds with different functional groups: haloalkanes, alcohols, ethers, aldehydes and ketones; carboxylic acids, esters and amines.
7.5 Proteins, polysaccharides and lipids.
7.6 Organic compounds in food. Detergents. Pesticides.

Mandatory literature

Sawyer, Clair N.; Chemistry for environmental engineering and science. ISBN: 0-07-119888-1
Atkins, Peter; Princípios de química. ISBN: 85-7307-739-5
Atkins, Peter; Chemical principles. ISBN: 0-7167-5701-X

Complementary Bibliography

Manahan, Stanley E.; Fundamentals of Environmental Chemistry

Teaching methods and learning activities

General theoretical-practical lectures (TPG)
Presentations supported by audiovisual media, and illustrated with the solution of problems related with practical examples, included in tutorial handouts to be delivered to the students. Special attention will be given to the application of knowledge in quotidian life issues, with interfaces with environment and Environmental Engineering. Students will be strongly stimulated to participate during the classes. Presences will be registered.

Theoretical-practical lectures for classes (TPT)
Besides the problems solved in TPG, the handouts will include proposals for problems to be solved in TPT, and other problems to be solved out of the classes, to facilitate learning and to consolidate knowledge. Special attention will be given to the critical analysis of results and to the search of data in tables delivered to the students. Absences will be registered.

Evaluation Type

Distributed evaluation without final exam

Assessment Components

Description	Type	Time (hours)	Weight (%)	End date
Subject Classes	Participação presencial	84,00
	Exame	1,50		2009-11-13
	Exame	2,00		2010-01-12
	Exame	2,50		2010-02-05
	Total:	-	0,00

Eligibility for exams

General rules

Calculation formula of final grade

Three evaluation assays.
The final classification (CF) of students, since they reach the minimum level of attendance to classes, will be calculated through the following equation:

CF = 0,20 * T1 + 0,35 * T2 + 0,45 * T3

where T1, T2 and T3 correspond to the classification of the three evaluation assays.
A minimum of 6.0/20.0 in each of the three assays is required for approval.

For the students that obtain a final mark <10 in the distributed evaluation, the final mark will be that obtained in a special exam.

Examinations or Special Assignments

Not applicable.

Special assessment (TE, DA, ...)

Final examination according to general rules.

Classification improvement

Not applicable.