Introduction à la relativité restreinte : Cours et exercices by Jean Hladik, Michel Chrysos

By Jean Hladik, Michel Chrysos

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2 gives some examples of Brønsted—Lowry acids and their conjugate bases. For all these pairs, we are dealing with the transfer of a hydrogen ion (proton) from the acid to some other species (often the solvent) to form the conjugate base. A convenient means of measuring the hydrogen ion concentration in aqueous solutions is the pH scale. 8) Consider the dissociation of a weak Brønsted—Lowry acid (HA) into a proton (H>) and its conjugate base (A\) in aqueous solution. HA & H> ; A\ The dissociation constant for the acid, K , is given by the ratio [H>][A\]/ ?

15, we see that the velocity for this reaction depends linearly on initial reactant concentration. 5 Reaction order for a few simple chemical reactions Order Reaction Rate Equation 1 2 2 A;P 2A ; P A;B;P v : k[A] v : k[A] v : k[A][B] constant. 24) A reaction of this type would be said to be a second-order reaction. Generally, the order of a chemical reaction is the sum of the exponent terms to which reactant concentrations are raised in the velocity equation. 5. , Atkins, 1978). As we have just seen, reactions involving two reactants, such as A ; B ; P, are strictly speaking always second order.

Molecules can interact with one another by a number of noncovalent forces as well. These weaker attractive forces are very important in biochemical reactions because they are readily reversible. , substrates and inhibitors) is a critical aspect of both enzymatic catalysis and enzyme inhibition. Four types of noncovalent interaction are particularly important in protein structure (Chapter 3) and enzyme—ligand binding (Chapters 4, 6, and 8); these are electrostatic interactions, hydrogen bonding, hydrophobic interactions, and van der Waals forces.

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