The lattice enthalpy of an ionic compound MX is `DeltaH_(L)` and the total enthalpy of hydration of `M^(+) and X^(-)` ions is `DeltaH_(hyd)`. Show that heat of solution of this ionic compound `DeltaH_(sol)=DeltaH_(L)+DeltaH_("hyd")`.

What do you mean by enthalpy? Show that DeltaH= DeltaU + Delta nRT .

The standard enthalpy of combustion of C_(x)H_(y)(l) at 25^(@)C is Q kJ*mol^(-1) . Write down the thermochemical equation for the combustion reaction of this compound.

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 .

For the salt CaF_(2),DeltaH_("lattice")^(0) gt DeltaH_("hyd")^(0) . Predict whether this salt is soluble in water or not.

Between O_(2)(g) and O_(3)(g) , whose standard enthalpy of formation (DeltaH_(f)^(0)) is taken as zero at 1 atm and 25^(@)C ?

In which of the following reactions does DeltaH^(0) at 25^(@)C indicate the standard enthalpy of formation (DeltaH_(f)^(0)) of the compound formed in each of the reactions? (2) N_(2)(g)+3H_(2)(g)to2NH_(3)(g) (2) (1)/(2)N_(2)(g)+(1)/(3)O_(3)(g)toNO(g) .

Why do halogens have high electron gain enthalpies (-Delta_H)?

At a certain temperature and pressure, DeltaH=0 for the reaction: X+X= X_(2) . Show that the reaction is non-spontaneous at this temperature and pressure.

A crystalline ionic compound consisting of M^(+)andX^(-) ions crystallises in cubic structure. The unit cell of the compound has M^(+) ions at its corners and an X^(-) ion at its body centre. Determine the simplest formula of the compound.