Download Basic physical chemistry for the atmospheric sciences by Peter V. Hobbs PDF

By Peter V. Hobbs

Up-to-date and revised, this hugely winning textual content information the fundamental chemical rules required for contemporary stories of atmospheres, oceans, and Earth and planetary structures. This thoroughly available advent permits undergraduate and graduate scholars with little formal education in chemistry to understand such primary techniques as chemical equilibria, chemical thermodynamics, chemical kinetics, answer chemistry, acid and base chemistry, oxidation-reduction reactions, and photochemistry. within the spouse quantity advent to Atmospheric Chemistry (also to be released in could 2000), Peter Hobbs information atmospheric chemistry itself, together with its purposes to pollution, acid rain, the ozone gap, and weather swap. jointly those books provide a great creation to atmospheric chemistry for numerous disciplines.

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Chemical thermodynamics 21 where dQ is the heat added to the system , dU the increase in internal energy of the system, and pdV the work done by the system when its volume increases by dV. For the air parcel dQ = 1 07 J and pdV = ( 1 . 0 1 3 x 1 05)(22) 0 . 22 x 1 07 J. Therefore , = dU = dQ - pdV = 1 07 - 0 . 8 x 1 06 J If the molecules in the air exer< no forces on each other, the internal energy of the air must consist entirely of the kinetic energy of the molecules , that is, on the temperature of the air.

E) Water can freeze spontaneously below 0°C even though this produces a decrease in the entropy of the system. (f) Some exothermic chemical reactions do not occur spon­ taneously. (g) List some spontaneous processes that are not exo­ thermic. (h) All chemical compounds will dissociate into the ele­ ments at sufficiently high temperatures. ) (i) Neither the heat absorbed (or released) nor the work Chemical thermodynamics 2. 1 1 . 2. 1 2 . done by (or on) a system i s a function of state, but the difference between these two quantities , namely , the change in the internal energy of a system , is a function of state .

From a molecular viewpoint, the disorder is associated with the molecules of a system . As in the case of energy or enthalpy , we are usually interested in differences in entropy rather than absolute values . However, in the case of entropy , it is possible to assign absolute value s. This is a consequence of the third law of thermodynamics , which states that the entropy of perfect crystals of all pure elements and compounds is zero at the absolute zero of temperature (0 K). Consequently , the absolute entropy of a substance at any temperature T is given by the change in the entropy of the substance in moving from 0 K to T.

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