Transcript Lecture I
CML100 • CML110 – Introduction to Chemistry [3 cr. (3-0-0)] • Semester II, 2014-2015, TuWF 10-10.50, 33.50 • Instructors: Dr. Shashank Deep (SD), Prof. Anil J. Elias (AJE) and Prof. Nalin Pant (NP) • Course Coordinator: Dr. Shashank Deep (SD) • Office: MS731 (SD) • Phone: 6596 (SD) • E-mail: [email protected] (SD) CYL 110 Grading • Grading based on: • • • • • Minor Tests I Minor Tests II 10 Home Assignments Major Test Passing grade is 30%. 25% 25% 10% 40% Recommended books • Books and Reference Material: • (i) Physical Chemistry by Atkins and de Paula • (ii) The Elements of Physical Chemistry by Atkins • (iii) Physical Chemistry by Silbey and Alberty • (iv) Physical Chemistry by Levine • (vi) Physical Chemistry: A Molecular Approach by McQuarrie and Simon • (vii) Physical Chemistry by Laidler, Meiser, and Sanctuary Course contents (Chemical Thermodynamics) • Revisit: Real gases, van der Waals and virial equations of state, Critical point. Zeroth and First law of themodynamics, internal energy, Exact and inexact differentials, Isothermal and adiabatic processes, Enthalpy, Heat Capacities. • Second law of thermodynamics and entropy, entropy changes in reversible and irreversible processes. Course contents (Chemical Thermodynamics) • Combined first and second law, thermodynamic potentials, free energy and work, effect of temperature and pressure on free energy. • Chemical potential, equilibrium and free energy, phase equilibria: phase rule, phase equilibrium of onecomponent system, clapeyron equation, clausius clapeyron equation, colligative properties. • Gaseous equilibrium, Le Chatelier’s principle, van’t Hoff equation. CYL110 Tutorials • http://web.iitd.ac.in/~sdeep • Menu Courses CML100 Thermodynamics • Effects of gravitational field, centrifugal field and surface area on the properties of the system. • Phase transitions like graphite to diamond conversion, helium normal to superfluid transition, conductor to semiconductor transition, change of boiling point of a liquid with pressure or addition of solute. • Biochemistry-Enzymes and protein stability, DNA stability, metabolic processes leading to mechanical work performed by a living organism, design of drugs. Thermo---------• Industrial Chemistry-Different chemical processes like synthesis of ammonia from nitrogen and hydrogen. • Thermodynamics of complexation with macrocyclic ligands- A system of interest in Inorganic chemistry and chemical separation. • Geological problems- solubility of calcite, energetics of ternary oxides of minerological significance. A thermodynamic system is that portion of the Universe that we have selected for investigation •The surroundings are everything outside the system. The boundary separates the system from the surroundings The state of a system is defined as the complete set of all its properties which can change during various specified processes. When a system is at equilibrium, its state is defined entirely by the state variables, and not by the history of the system. The properties of the system can be described by an equation of state which specifies the relationship between these variables. System-------------------------- GAS Variables---------------------- n, P,V,T Equation of State -------- PV=nRT A perfect gas is defined as “A gas where intermolecular forces are negligible”. Temperature • Zeroth law of thermodynamics. • Do we need definition of temperature ? • On a cold winters day a metal railing feels much colder than a wooden fence post, but they are both at the same temperature. • The zeroth law states “If two systems are separately in thermal equilibrium with a third, then they must also be in thermal equilibrium with each other.” Ideal Gas Model • Molecules may be treated as point masses relative to the volume of the system. • Molecular collisions are elastic, i.e. kinetic energy is conserved. • Intermolecular forces of attraction and repulsion have negligible effect on the molecular motion. Compressibility • The compressibility of a gas is defined by pVm Z RT • If the gas behaves ideally, then Z=1 at all pressures and temperatures. • Z >1 molecules occupy more volume than IG (e.g. H2): repulsive forces • Z < 1 molecules occupy less volume than IG (e.g. CO2): attractive forces Boyle’s temperature Z 0 P T Z 0 1 V m B0 as P0 as V Critical constants of some gases • The very low critical pressure and temperature of helium, reflecting the very small intermolecular attractions of this atom. • Tc of the noble gas elements increases with atomic number. • Hydrogen gas cannot be liquified above 33 K; this poses a major difficulty in the use of hydrogen as an automotive fuel; storage as a high-pressure gas requires heavy steel containers which add greatly to its effective weight-per-joule of energy storage. • The properties of carbon dioxide (particularly its use as a supercritical fluid). • The high Tc of H2O is another manifestation of its "anomalous" properties relating to hydrogen-bonding. Calculation of critical point a point on a curve at which the tangent crosses the curve itself. a point on a curve at which the curvature changes sign. A point on a curve at which the second derivative changes sign. a point (x,y) on a function, f(x), at which the first derivative, f'(x), is at an extremum, i.e. a minimum or maximum. Virial equation of state It is based on statistical mechanical theory, where each power level indicates a higher level of interaction. The virial equation does not tend to be very good at high densities (low T, high P). van der Waals Equation p a / V V 2 m m b nRT Vm,eff Vm b repulsion peff p a / V attraction 2 m van der Waals constants a (dm6 atm mole-1) b (dm mole-1) He 0.034 0.0237 Ar 1.345 0.0322 N2 1.390 0.0391 O2 1.360 0.0318 CO2 3.592 0.0427