Class Introduction to Physical Chemistry

Introduction to Physical Chemistry aims to provide students with the knowledge necessary to understand the importance of physical processes in biochemistry. Biological systems have some constraints imposed by their environment. This course aims to identify and understand the constraints that physics and chemistry impose on biological systems.

1.Gases
1.1.Perfect gases
1.1.1.Gases laws.
1.2. Real Gases.
1.2.1.Molecular interactions.
1.2.2.van der Waals Equation.
1.3. Environmental impact. Mitigating enzymes.
2.Thermodynamics.
2.1. First law.
2.1.1.Internal energy, worl and heat.
2.1.2.Reversible versus irreversible processes.
2.1.3. Enthalpy.
2.1.4 Hess law, Enthalpy of formation
2.1.5.Heat Capacity.
2.2. Second law of thermodynamics. Entropy
2.3. Third law of Thermodynamics
2.3.1. Reaction Entropy. Gibbs energy.
2.4. Chemical equiibrium. Changes in Gibbs energy.
2.4.1.Equilibrium constant. van't Hoff Equation.
3. Electrochemistry.
3.1.Standard Reduction PotentialPotencial.
3.2.Nernst equation; equilibrium constant determination.
4. Kinetics.
4.1.Reaction rates.Reaction order.
4.2.Integrated rate laws.
4.4. Steady-sate.
4.5. Enzimatic catalysis. Arrhenius equation.

In this CU, students carry out individual and group work in order to work as a team. Practical classes are very intertwined with theoretical classes so that students understand the importance of Physical-Chemistry  in understanding biological systems.

• Paula, J. and Atkins, P. (2010), Atkins' Physical Chemistry, 9 edition, Oxford edition
• Paula, J. and Atkins, P. (2006), Physical Chemistry for the Life Sciences, 2 edition, W.H. Freeman and Company