Combustion of sucrose is used by aerobic organisms for providing energy for the life substaining process. If all the capturing from the reaction is done through electrical process (non P-V work) then calculate maximum available energy which can be captured by combustion of 34.2 gm of sucrose Given :
`Delta H_("sucrose") = -6000 kJ mol^(-1) , Delta S_("combustion") = 180 J// K mol` and body temperature is 300 K.
Combustion of sucrose is used by aerobic organisms for providing energy for the life substaining process. If all the capturing from the reaction is done through electrical process (non P-V work) then calculate maximum available energy which can be captured by combustion of 34.2 gm of sucrose Given :
`Delta H_("sucrose") = -6000 kJ mol^(-1) , Delta S_("combustion") = 180 J// K mol` and body temperature is 300 K.
`Delta H_("sucrose") = -6000 kJ mol^(-1) , Delta S_("combustion") = 180 J// K mol` and body temperature is 300 K.
A
600 kJ
B
`594.6` kJ
C
`5.4` kJ
D
605.4 kJ
Text Solution
Verified by Experts
The correct Answer is:
D
No. of moles of surcose `=(34.2)/(342)=0.1`
`-(DeltaG)_(T,P)` = useful work done by the system
`DeltaG=-DeltaH+T.DeltaS`
`=+(6000xx0.1)+(180xx0.1xx300)/(1000)`
= 605.4 kJ
`-(DeltaG)_(T,P)` = useful work done by the system
`DeltaG=-DeltaH+T.DeltaS`
`=+(6000xx0.1)+(180xx0.1xx300)/(1000)`
= 605.4 kJ
Topper's Solved these Questions
Similar Questions
Explore conceptually related problems
The change in Gibbs free energy of the system along provides a criterion for the spontaneity of a process at constant temperature and pressure. A change in the free energy of a sytem at constant temperature and pressure will be: DeltaG_("system") = DeltaH_("system") - T DeltaS_("system") The free energy for a reaction having Delta H= 31400 cal, DeltaS= 32 cal K^(-1) mol^(-1) at 1000^(@)C is
Liquid water freezes at 273K under external pressure of 1 atm. The process is at equilibrium H_(2)O (l) hArr H_(2)O (s) at 273 K & 1 atm. However it was required to calculate the thermodynamic parameters of the fusion process occuring at same pressure & different temperature.Using the following data, answer the question that follow. d_("ice") = 0.9 gm/cc, d_(H_(2)O(l)) = 1 gm//c, C_(P) [H_(2)O(s))] = 36.4 JK^(-1) mol^(-1) C_(P) [H_(2)O(l)] = 75.3 JK^(-1) mol^(-1), Delta H_("fusion") = 6008.2 J mol^(-1) The value of '' Delta H_("fusion") '' at 263K & 1 atm will be
Liquid water freezes at 273K under external pressure of 1 atm. The process is at equilibrium H_(2)O (l) hArr H_(2)O (s) at 273 K & 1 atm. However it was required to calculate the thermodynamic parameters of the fusion process occuring at same pressure & different temperature.Using the following data, answer the question that follow. d_("ice") = 0.9 gm/cc, d_(H_(2)O(l)) = 1 gm//c, C_(P) [H_(2)O(s))] = 36.4 JK^(-1) mol^(-1) C_(P) [H_(2)O(l)] = 75.3 JK^(-1) mol^(-1), Delta H_("fusion") = 6008.2 J mol^(-1) '' DeltaS_("fusion") '' at 263 K & 1 atm will be
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
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) The heat capacity of bomb calorimeter (with its contents) is 500J/K. When 0.1g of CH_(4) was burnt in this calorimeter the temperature rose by 2^(@)C . The value of DeltaU per mole will be
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