Which formulate in the following are correct?
a) `G=H-TS`
b) `DeltaG_("sys")=DeltaH_("sys")-TDeltaS_("sys")`
c) `DeltaS_("surr")=(DeltaH_("surr"))/(T)=(-DeltaH_("sys"))/(T)`
d)`DeltaS_("total")=DeltaS_("sys")+((-DeltaH_("sys")))/(T)`
e) `DeltaS_("total")=TDeltaS_("sys")-DeltaH_("sys)`

Delta G_(sys) is equal to

For which of the following cases DeltaS = (DeltaH)/T

DeltaG = DeltaH-TdeltaS and DeltaG = DeltaH + T[(d(DeltaG))/(dT)] " then " ((dE_("cell"))/(dT)) is

For isothermal expansion of an ideal gas into vacuum, among the following how many are zero, Pext, g, Delta T, Delta U, Delta H, Delta S, Delta G, Delta S_("surr"), Delta S_("total")

Chemical reactions are invariably associated with the transfer of energy either in the form of hear or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called calorimeter. Heat change in the process is calculated as: q= ms Delta T , s= Specific heat = c Delta T = Heat capacity. Heat of reaction at constant pressure is measured using simple or water calorimeter. Q_(v)= Delta U = Internal energy change, Q_(P) = DeltaH, Q_(P) = Q_(V) + P Delta V and DeltaH = Delta U+ Delta nRT . The amount of energy released during a chemical change depends on the physical state of reactants and products, the condition of pressure, temperature and volume at which the reaction is carried out. The variation of heat of reaction with temperature and pressure is given by Kirchoff's equation: (DeltaH_(2) - DeltaH_(1))/(T_(2)-T_(1))= Delta C_(P) (At constant pressure), (DeltaU_(2) - DeltaU_(1))/(T_(2)-T_(1)) = DeltaC_(V) (At constant volume) The enthalpy change (DeltaH) for the reaction N_(2) (g) + 3H_(2)(g) rarr 2NH_(3)(g) is -92.38kJ at 298 K. The internal energy change DeltaU at 298 K is

Chemical reactions are invariably assocated with the transfer of energy either in the form of heat or light. In the laboratory, heat changes in physical and chemical processes are measured with an instrument called calorimeter. Heat change in the process is calculated as: q= ms DeltaT , s= specific heat = c Delta T , c= heat capacity Heat of reaction at constant volume is measured using bomb calorimeter. qv= Delta U= internal energy change. Heat of reaction at constant pressure is measured using simple or water calorimeter. q_(p) = Delta H, q_(p) = q_(v) + P Delta V, DeltaH = DeltaU + Delta nRT The amount of energy released during a chemical change depnds on the physical state of reactants and products, the condition of pressure, temperature and volume at which the reaction is carried out. The variation of heat of reaction with temperature and pressure is given by Kirchhoff's equation: (DeltaH_(2)- DeltaH_(1))/(TT_(2)-T_(1)) = DeltaC_(P) (At constant pressure), (DeltaU_(2)- DeltaU_(1))/(TT_(2)-T_(1)) = DeltaC_(V) (At constant volume) DeltaC_(P) for a reaction is given by 0.2T cal/deg. Its enthalpy of reaction at 10K is -14.2 kcal. Its enthalpy of reaction at 100K in kcal will be

Two compounds form an ideal solution at room temperature. Which of the following are correct for this ideal solution ? (a) Delta G =+ ve (b) Delta S =+ ve surrounding (c ) Delta S = + vc system (d) Delta _(mix) H=0

Two compounds form an ideal solution at room temperature. Which of the following are correct for this ideal solution? (A) Delta G = ( + ve) (B) Delta S = (+ ve) surrounding (C ) Delta S = (+ve) system (D) Delta_(max) H = 0