[" 1.The specific heats of iodine vapour and solid are "0.031" and "],[Delta6" 0.055callg respectively.If heat of sublimation of iodine is "],[" Deltau "24" callg at "200^(@)C" ,what is its value at "250^(@)C" ? "]

The specific heats of iodine vapour and solid are 0.031 and 0.055 cal//g respectively. If heat of sublimation of iodinde is 24cal//g at 200^(@)C , what is its value at 250^(@)C ?

The specific heats of iodine vapour and solid are 0.031 and 0.055 cal//g respectively. If heat of sublimation of iodinde is 24cal//g at 200^(@)C , what is its value at 250^(@)C ?

Heat of reaction is the change in enthalpy or internal energy as represented by a balanced thermochemical equation . The amount of energy released during a chemical change depends upon the state of reactants and products, the conditions of pressure and volume at which reaction is carried out, and temperature. The variation of heat of reaction (DeltaH_(1) or DeltaE) with temperature is given as DeltaH_(2)-DeltaH_(1)=DeltaC_(P)[T_(2)-T_(1)] or DeltaE_(2)-DeltaE_(1)=DeltaC_(v)(T_(2)-T_(1). Standard heat enthalpy of elements in their most stable state is assumed to be zero whereas standard heat enthalpy of compound is referred as heat of formation of that compound at 1 atm pressure and 25^(@)C . Oxidation of N_(2) to N_(2)O,NO,NO_(2) shows absorption of energy whereas heat of combustion of N_(2) is exothermic like other heat of combustion. The specific heat of I_(20 in vapour and solid state are 0.031 and 0.55cal//g respectively. If heat of sublimation of iodine is 6.096 kcal mol^(-1) at 200^(@)C , the heat of sublimation of I_(2) at 250^(@)C is :

The specific heat of ice at 0^@C is

The specific heat of ice at 0^(@)C is

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 specific heat of I_(2) in vapoour and solid state are 0.031 and 0.055 cal/g respectively. The heat of sublimation of iodine at 200^(@)C is 6.096 kcal mol^(-1) . The heat of sublimation of iodine at 250^(0)C will be