Home
Class 11
CHEMISTRY
Heat of reaction (DeltaH) is given by...

Heat of reaction `(DeltaH)` is given by

A

`DeltaH` = Activation energy of forward reaction - Activation energy of backward reaction

B

`DeltaH` = Sum of bond energy of reactants - Sum of bond energy of products

C

`DeltaH` = Sum of enthalpy of products - Sum of enthalpy of reactants

D

All the above

Text Solution

Verified by Experts

The correct Answer is:
D
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE - 1 (ENTORPY AND GIBBS ENERGY)|42 Videos
  • CHEMICAL THERMODYNAMICS

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE - 2 (FIRST LAW OF THERMODYNAMICS)|10 Videos
  • CHEMICAL THERMODYNAMICS

    AAKASH SERIES|Exercise OBJECTIVE EXERCISE - 1 (OTHER HEATS OF REACTIONS)|7 Videos
  • CHEMICAL THERMODYANMICS

    AAKASH SERIES|Exercise Questions For Descriptive Answers|28 Videos
  • ELECTRON MIGRATION EFFECTS

    AAKASH SERIES|Exercise QUESTIONS FOR DESCRIPTIVE ANSWERS|10 Videos

Similar Questions

Explore conceptually related problems

Haloform reaction is not given by

For an endothermic reaction energy of activation is E_(a) and enthalpy of reaction is DeltaH (both in kJ "mol"^(-1) ) Minimum value of E_(a) will be

Calculate the heat of formation (DeltaH) of CO from the following data. (I) C_(graph ite)+2H_(2)(g)toCH_(4)(g)," " DeltaH=-94kcal (II) CO(g)+(1)/(2)O_(2)toCO_(2)(g)," "DeltaH=-68kcal

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

For the reaction, N_(2(g)) + 3H_(2(g)) rarr 2NH_(3(g)) . Heat of reaction at constant volume exceeds the heat of reaction at constant pressure by the value of xRT. The value of x is______

Change in enthalpy and change in internal energy are state functions. The value of DeltaH, DeltaU can be determined by using Kirchoff's equation. Calculate the heat of formation of methane, given that heat of formation of water = -286kJ mol^(-1) , heat of combustion of methane = -890kJ mol^(-1) heat of combustion of carbon = -393.5 kJ mol^(-1)