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For a reaction involving condensed phase...

For a reaction involving condensed phases, `DeltaH = DeltaU`.

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The enthalpy change for chemical reaction is denoted aas DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal enegry is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry Deltan = change in number of moles, R = gas constant. For a reaction, 2X(s) +2Y(s) rarr 2C(l) +D(g), DeltaH at 27^(@)C is -28 kcal mol^(-1). DeltaU is ..... kcal mol^(-1)

The enthalpy change for chemical reaction is denoted as DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal energy is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal energy Deltan = change in number of moles, R = gas constant. Enthalpy of the system is given as

The enthalpy change for chemical reaction is denoted as DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal enegry is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry Deltan = change in number of moles, R = gas constant. For the change, C_("diamond") rarr C_("graphite"), DeltaH =- 1.89 kJ , if 6g of diamond and 6g of graphite are seperately burnt to yield CO_(2) the heat liberated in first case is

The enthalpy change for chemical reaction is denoted aas DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal energy is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal energy Deltan = change in number of moles, R = gas constant. Which of the following equations corresponds to the definition of enthalpy of formation at 298K ?

The enthalpy change for chemical reaction is denoted aas DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal enegry is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry Deltan = change in number of moles, R = gas constant. Enthalpy of the system is given as

The enthalpy change for chemical reaction is denoted aas DeltaH^(Theta) and DeltaH^(Theta) = H_(P)^(Theta) - H_(R)^(Theta) . The relation between enthalpy and internal energy is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry Deltan = change in number of moles, R = gas constant. H_(2)(g) +((1)/(2))O_(2)(g) = H_(2)O(l), DeltaH_(298K) = - 68.00kcal Heat of voporisation of water at 1 atm and 25^(@)C is 10.00 kcal . The standard heat of formation (in kcal) of 1 mole vapour a 25^(@)C is

Define enthalpy. Show that the change in enthalpy at constant pressure for a reaction involving gases is given by the expression, DeltaH = DeltaU + Deltan_(g) .RT .

Under which of the following condition is the relation DeltaH = DeltaU +P DeltaV valid for a closed system at

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State a chemical reaction in which DeltaH and DeltaU are equal .

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