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

By Peter V. Hobbs

ISBN-10: 052147387X

ISBN-13: 9780521473873

ISBN-10: 0521479339

ISBN-13: 9780521479332

Up-to-date and revised, this hugely winning textual content info the fundamental chemical rules required for contemporary experiences of atmospheres, oceans, and Earth and planetary platforms. This thoroughly available creation permits undergraduate and graduate scholars with little formal education in chemistry to understand such basic options 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 may well 2000), Peter Hobbs info atmospheric chemistry itself, together with its functions to pollution, acid rain, the ozone gap, and weather swap. jointly those books provide a great creation to atmospheric chemistry for a number of disciplines.

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Basic physical chemistry for the atmospheric sciences

Up to date and revised, this hugely profitable textual content info the elemental chemical ideas required for contemporary experiences of atmospheres, oceans, and Earth and planetary structures. This thoroughly available advent permits undergraduate and graduate scholars with little formal education in chemistry to know such basic ideas as chemical equilibria, chemical thermodynamics, chemical kinetics, answer chemistry, acid and base chemistry, oxidation-reduction reactions, and photochemistry.

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Sample text

I t follows from the above definitions and Eq . (2. 32) that i f LlGjl(X) for a reaction is negative, the reactants in their standard states will be converted spontaneously into the products in their standard states. If LlGJ is positive , the conversion will not be spontaneous , but the corresponding reverse reaction will be . However, even when LlGJ is positive , some products can form but in concentrations below that of their standard states . 6. Oz(g) Is H 2 0z(g) stable at 25°C and 1 atm? Solution .

2 . 28) and (2 . e . e . , an increase in the entropy of a system) . These results can be summarized as follows . The transformation of a system from one state to another, at constant temperature and pressure, is spontaneous if the Gibbs free energy (of the system alone) decreases . If the Gibbs free energy (of the system alone) is unchanged by th e transformation , the two states are in equilibrium . In other words, the criterion for the thermodynamic equilibrium of a system at constant temperature and pressure is that the Gibbs free energy of the system be at a minimum value.

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 .

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


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