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THERMODYNAMICS

CHEMISTRY154 THERMODYNAMICSIt is the only physical theory of universal content concerningwhich I am convinced that, within the framework of theapplicability of its basic concepts, it will never be EinsteinAfter studying this Unit, you willbe able to explain the terms : system andsurroundings; discriminate between close,open and isolated systems; explain internal energy, workand heat; state first law ofthermodynamics and expressit mathematically; calculate energy changes aswork and heat contributionsin chemical systems; explain state functions: U, H. correlate DU and DH; measure experimentally DUand DH; define standard states for DH; calculate enthalpy changes forvarious types of reactions; state and apply Hess s law ofconstant heat summation; differentiate between extensiveand intensive properties; define spontaneous and non-spontaneous processes; explain entropy as athermodynamic state functionand apply it for spontaneity; explain Gibbs energy change(DG); establish relationship betweenDG and spontaneity, DG andequilibrium energy stored by molecules can be released as heatduring chemical reactions when a fuel like methane, cookinggas or coal burns in air.

2. Closed System In a closed system, there is no exchange of matter, but exchange of energy is possible between system and the surroundings [Fig. 6.2 (b)]. The presence of reactants in a closed vessel made of conducting material e.g., copper or steel is an example of a closed system. Fig. 6.2 Open, closed and isolated systems.

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