In the relation `DeltaH = DeltaU + (Deltan_(g))RT` the units of `Deltan_(g)` is mol.

The relation between DeltaU and DeltaH :

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 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 enegry 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 amol vapour a 25^(@)C 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 enegry is expressed by equation: DeltaH = DeltaU +DeltanRT where DeltaU = change in internal enegry 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

In the relation, K_(p)=K_(c)(RT)^(Deltan) the value of Deltan is

Unit of K_(p) is (atm)^(Deltan)

Assertion (A) : For gaseous reaction when Delta n =0 , K_(p)=K_(c) . Deltan = change in the number of gas moles Reason (R ) : For gaseous reaction, K_(p)=K_(c)(RT)^(Deltan)