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Heat of reaction at constant pressure is...

Heat of reaction at constant pressure is………….. .

A

`Delta U`

B

`Delta H`

C

`Delta P`

D

`Delta V`

Text Solution

Verified by Experts

The correct Answer is:
B
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Chemical reactions are invariably associated with the transfter 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),(=cDeltaT,,c =Heat capacity):} Heat of reaction at constant volume is measured using bomb calorimeter. q_(V) = DeltaU = Internal energy change Heat of reaction at constant pressure is measured using simple or water calorimeter. q_(p) = DeltaH q_(p) = q_(V) +P DeltaV DeltaH = DeltaU +DeltanRT For which reaction will DeltaH = DeltaU ? Assume each reaction is carried out in an open container.

Chemical reactions are invariably associated with the transfter 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"),(=cDeltaT,,c ="Heat capacity"):} Heat of reaction at constant volume is measured using bomb calorimeter. q_(V) = DeltaU = Internal energy change Heat of reaction at constant pressure is measured using simple or water calorimeter. q_(p) = DeltaH q_(p) = q_(V) +P DeltaV DeltaH = DeltaU +DeltanRT The heat capacity of a bomb calorimeter is 500 JK^(-1) . When 0.1g of methane was burnt in this calorimeter, the temperature rose by 2^(@)C . The value of DeltaU per mole will be

Knowledge Check

  • Heat of a reaction (Q) at constant pressure is equal to

    A
    `E_(P)-E_(R)`
    B
    `E_(R)-E_(P)`
    C
    `H_(P)-H_(R)`
    D
    `H_(R)-H_(P)`

  • what the heat of a reaction at constant pressure is -2.5 xx 10^(3) cal and entropy change for the reaction is 7.4cal deg ^(-1) , it is predicted that the reaction at 25^(@)C is

    A
    reversible
    B
    spontaneous
    C
    non-spontaneous
    D
    irreversible

  • Chemical reactions are invariable associated with the transfer of enery either in the form of heat or light. In the laboratory, heat energy I physical and chemical processes are measured with an instrument called caloriemter. Heat change in the process is calcualted as: q-msDeltaT," "s= specific heat =cDeltaT," "c= Heat capacity. Heat of reaction at constant pressure is measured using bomb calorimeter. q_(V)=DeltaU= Internal energy change heat of reaction at constant pressure is measrued using simple or water calorimeter. q_(P)=DeltaH q_(P)=q_(V)+PDeltaV DeltaH=DeltaU+DeltanRT The amount of energy released during a chemical change depends on the physical state of reactants and products, te conditions of pressure, temperatrue 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))/(T_(2)-T_(1))=DeltaC_(P)," "(DeltaU_(2)-DeltaU_(1))/(T_(2)-T_(1))=DeltaC_(V) . Q. The specific heats of I_(2) in vapour and solid states 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^(@)C will be:

    A
    3.8 kcal `mol^(-1)`
    B
    4.8 kcal `mol^(-1)`
    C
    `2.28` kcal `mol^(-1)`
    D
    5.8 kcal `mol^(-1)`

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