Chemistry Basic Elements by Augustus Bailey

By Augustus Bailey

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879 JK_1 Shown that for an ideal gas undergoing isothermal reversible expansion, DG = DA. 19 mm Hg. 19 mm Hg will be reversible in nature. Thus DG for this process will be equal to zero. 4 J mole_1 Trouton's rule concerning entropy of vapourization. u. By a normal liquid, we mean which is not associated. In general association in the liquid state may be expected when intermolecular forces of a dominant type operate. , lead to this situation. Abnormally high boiling points are a consequence of molecular association in the liquid state.

Of moles. Matched : (a) Isothermal process (1) when P = constant (b) Adiabatic process (2) when heat capacity of body = constant (c) Isobaric process (3) when dE = dH = 0 (d) Polytropic process (4) when T = constant (e) Quasistatic process (5) when both E and H = constant (f) Isochoric process (6) when q = constant (g) Cyclic process (7) when V = constant (a) 4, (b) 6, (c) 1, (d) 2, (e) 3, (f) 7, (g) 5. A psychologist develops a theory that states of mind (anger, suspicion, greed) are thermodynamic states of a region of the brain that can be considered a system.

9 × 100 = 90 T1 = 90 per cent of T2 Without doing calculations, the signs of Dp, DV, DT, DE, DH and DS for one mole of an ideal gas calculated taken through each of the following four steps of a Carnot cycle. Cp and CV as constants assumed : Step (1) Isothermal reversible expansion p1, V1, Tl ® p2, V2, T2 Step (2) Adiabatic reversible expansion p2, V2, T1 ® p3, V3, T2 Step (3) Isothermal reversible compression p3, V3, T2 ® p4, V4, T2 Step (4) Adiabatic reversible compression p4, V4, T2 ® p1, V1, T1 Chemical Equilibrium Step (1): DV = +ve as expansion takes place DT = 0 as process is isothermal Dp = _ve as increase in volume at constant temperature will decrease the pressure (Boyle's law) DE = 0 since for an ideal gas E = f (T) & DT = 0 DH = 0 DH = DE + D(pV) and DE = 0 and D(pV) = D(RT) = 0 DS = +ve since DS = nR In V2 > V1 and Step (2): DV = +ve as expansion takes place DS = 0 as adiabatic process is reversible DE = _ ve since DE = w & w is _ ve (expansion process) DT = _ ve since DE = Cv, m (DT) DH = _ ve since DH = DE + D(pV) = DE + RDT DP = _ ve Step (3) : Here the signs will be just opposite to those listed in step (1).

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