Biology 1001A Chapter Notes - Chapter 2: Calorimetry, Single Bond, Bond Order

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Enthalpy (h) an extensive property and state function, is the energy content of a system at constant pressure. Like internal energy, absolute enthalpy cannot be measured, but changes in enthalpy can. At (cid:272)o(cid:374)sta(cid:374)t p(cid:396)essu(cid:396)e, the h of a s(cid:455)ste(cid:373) is e(cid:395)ual to the heat (cid:894)(cid:395)p) flowing into or out of a system. E(cid:374)thalp(cid:455) u(cid:374)de(cid:396) sta(cid:374)da(cid:396)d (cid:272)o(cid:374)ditio(cid:374)s a(cid:396)e (cid:396)epo(cid:396)ted as ho. Latent heat is the energy change associated with physical processes that involve a change of state (phase) Forward and reverse processes have q values of the same magnitude but of opposite signs. The standard enthalpy change for a reaction is the difference between the sums of the standard, absolute molar enthalpies of the products and those of the reactants. If a (cid:396)ea(cid:272)tio(cid:374) is e(cid:454)othe(cid:396)(cid:373)i(cid:272), h<0 (cid:894)(cid:396)eleases heat(cid:895) If a (cid:396)ea(cid:272)tio(cid:374) is e(cid:374)dothe(cid:396)(cid:373)i(cid:272), h>0 (cid:894)a(cid:271)so(cid:396)(cid:271)s heat(cid:895) Calorimetry is used to study the heat flow of physical and chemical processes.

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