The heat of reaction at constant volume `(DeltaE)` and that at constant pressure `(DeltaH)` are related as

Define specific heat of a gas at constant volume and that at constant pressure.

(i) What do you mean by heat of reaction at constannt volume and heat of reaction at constant pressure? (ii) Establish the relation DeltaH=DeltaU=DeltanRT for a chemical reaction in gaseous state.

Show that the difference between the heat of reactionn at constant pressure (q_P or DeltaH) and that at constant volume (q_(V) or DeltaU) is PDeltaV .

The difference between heat of reaction at constant pressure (DeltaH) and at constant volume ( DeltaE ) for the reaction : C_((s))+(1)/(2)O_(2(g)) to CO_((g)) is :- (Assume R = 0.002 Kcal K^(-1) "mol"^(-1) and temperature =TK)

The heat of reaction at constant volume and temperature is represented by

For a reaction aA(g)hArrbB(g) at equilibrium, the heat of reaction at constant volume is 1500 cal more than at constant pressure. If the temperature is 27^(@)C then

For a reaction aA(g)hArrbB(g) at equilibrium, the heat of reaction at constant volume is 1500 cal more than at constant pressure. If the temperature is 27^(@)C then

For a reaction at constant temperature derive the relation between heat of reaction at constant pressure (Delta H) and heat of reaction at constant volume (Delta U) [considering ideal gas] .