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, and acetic acids; soda; potash; hydrogen carbonate ion; ammonia.

- Buffer solutions.

- Temporal 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 rate 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-life. Half-life of a radioactive nuclide. Documentary approach: using documents on radionuclides, address issues related to their use, storage, or reprocessing, for example.

- Arrhenius empirical law; activation energy.

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

Numerical approach: use the results of a numerical method to highlight approximations of the kinetically determining step or quasi-steady state.

• Identify the nature of reactions in aqueous solutions.
• Know how to 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 the dominant species.
• Know the nature (acidic/basic, strong/weak) of the most common examples cited above.
• Calculate the pH of a buffer solution, calculate the concentration of each chemical species in a buffer solution.
• Understanding the usefulness of buffer solutions.
• Extract relevant 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 whether a solution will be saturated or unsaturated, in solid or gas form.
• Use curves showing how solubility changes as a function of a variable.
• Determine the influence of a parameter on the speed of a chemical reaction. Relate the reaction speed, in cases where it is defined, to the speed at which a reactant disappears or a product is formed.
• Establish a velocity law based on the temporal 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 dates using a numerical or graphical method.
• Determine a reaction order using the differential method or half-reaction times or the integral method, strictly limiting yourself to a decomposition of order 0, 1, or 2 of a single reactant, or reducing to such a case by order degeneration or stoichiometric initial conditions.
• Determine the activation energy of a chemical reaction.
• Determine the activation energy of a chemical reaction based on kinetic constant values at different temperatures.
• Distinguish between the chemical equation symbolizing a chemical reaction and the equation representing an elementary act. Express the rate law of an elementary act. Plot an energy profile corresponding to an elementary act or to several successive elementary acts.
• Distinguishing between a reaction intermediate and an activated complex (transition state).
• Interpreting the role of the catalyst. Recognizing a catalytic effect in a reaction mechanism.
• Recognize the conditions for using the approximation of the kinetically determining step or the quasi-steady state.
• Establish the law governing the rate of disappearance of a reactant or formation of a product based on a simple reaction mechanism, using classical approximations where appropriate.

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

3 continuous assessments. Final grade = 20% CA1 + 30% CA2 + 50% CA3