• Level of study

    BAC +1

  • ECTS

    2 credits

  • Component

    Faculty of Science

Description

- 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.

- 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. Rate of reaction 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, address, for example, the problems related to their use, storage or reprocessing.

- Empirical Arrhenius law; activation energy.

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

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

 

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Objectives

  • Identify the nature of reactions in aqueous solutions.
  • Know how to construct and interpret a predominance diagram. Find the values of equilibrium constants by reading distribution curves and predominance diagrams (and vice versa). Use predominance or existence diagrams to predict incompatible species or the nature of the 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 usefulness of buffer solutions.
  • Extract, from available resources, relevant thermodynamic data 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 state of saturation or non-saturation of a solution, in solid or gas.
  • To exploit curves of evolution of the solubility according to a variable.
  • Determine the influence of a parameter on the rate of a chemical reaction. Relate the rate of reaction, where defined, to the rate of disappearance of a reactant or formation of a product.
  • Establish a law of velocity from the time tracking of a physical quantity.
  • Express the rate law if the chemical reaction has an order and determine the value of the kinetic constant at a given temperature.
  • Determine the rate of reaction at different dates using a numerical or graphical method.
  • Determine an order of reaction using the differential method or using 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 value of the activation energy of a chemical reaction from values of the kinetic constant at different temperatures.
  • Distinguish the chemical equation symbolizing a chemical reaction from the equation expressing an elementary act. To express the rate law of an elementary act. To draw an energy profile corresponding to an elementary act or to several successive elementary acts.
  • Distinguish a reaction intermediate from an activated complex (transition state).
  • Interpretation of the role of the catalyst. Recognize a catalytic effect in a reaction mechanism.
  • Recognize the conditions for using the kinetically deterministic 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 classical approximations.

 

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Necessary pre-requisites

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

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Knowledge control

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

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