General Chemistry 2 - Part 2

- Definition of an acid-base reaction.

- Acidity constant.

- Predominance diagram.

- Common examples of acids and bases: name, formula and nature - weak or strong - of sulfuric, nitric, hydrochloric, phosphoric, acetic acids, soda, potash, hydrogen carbonate ion, ammonia.

- Buffer solutions.

- Time evolution of a chemical system and reaction mechanisms in a closed reactor of uniform composition. Rates of disappearance of a reactant and formation of a product. Reaction rates for a transformation modeled by a single chemical reaction.

- Speed laws: reactions without order, reactions with simple order (0, 1, 2), global order, order

apparent.

- Half-reaction time. Half-life of a radioactive nuclide. Documentary approach: using documents on radionuclides, tackle issues such as their use, storage and reprocessing.

- Empirical Arrhenius law; activation energy.

- Reaction mechanisms. Elementary acts, molecularity, reaction intermediates, transition states. Kinetically decisive step, quasi-steady-state approximation (QSSA).

Numerical approach: use the results of a numerical method to demonstrate approximations of the kinetically decisive step or the quasi-stationary state.

• Identify the nature of reactions in aqueous solutions.
• Construct and interpret a predominance diagram. Find equilibrium constant values by reading distribution curves and predominance diagrams (and vice versa). Use predominance or existence diagrams to predict incompatible species or the nature of majority species.
• Know the nature (acid/base, strong/weak) of the most common examples listed above.
• Calculate the pH of a buffer solution, calculate the concentration of each chemical species in a buffer solution.
• Know the purpose of buffer solutions.
• Extract thermodynamic data from available resources to qualitatively predict the final state of a system in aqueous solution or to interpret experimental observations.
• Determine the value of the equilibrium constant for a reaction equation, which can be written as a linear combination of equations whose thermodynamic constants are known.
• Predict the saturation or non-saturation state of a solid or gas solution.
• Draw solubility curves as a function of one variable.
• Determine the influence of a parameter on the rate of a chemical reaction. Relate the reaction rate, where defined, to the rate at which a reactant disappears or a product is formed.
• Establish a speed law from the time tracking of a physical quantity.
• Express the rate law if the chemical reaction admits an order and determine the value of the kinetic constant at a given temperature.
• Determine the reaction rate at different times using a numerical or graphical method.
• Determine a reaction order using the differential method or half-reaction times or the integral method, strictly limited to a decomposition of order 0, 1 or 2 of a single reactant, or reducing to such a case by degeneracy of order or stoichiometric initial conditions.
• Determine the activation energy of a chemical reaction.
• Determine the activation energy of a chemical reaction from values of the kinetic constant at different temperatures.
• Distinguish between a chemical equation symbolizing a chemical reaction and an equation expressing an elementary act. Express the rate law of an elementary act. Draw an energy profile corresponding to an elementary act or to several successive elementary acts.
• Distinguish between a reaction intermediate and an activated complex (transition state).
• Interpret the role of the catalyst. Recognize a catalytic effect in a reaction mechanism.
• Recognize the conditions for using the kinetically decisive step or quasi-steady-state approximation.
• Establish the rate law for the disappearance of a reactant or the formation of a product from a simple reaction mechanism, possibly using standard approximations.

Stoichiometry, chemical formula, states of matter, elements of differential calculus. 

3 continuous tests. Final grade = 20% CC1 + 30% CC2 + 50% CC3