For a non-ideal solution, `Delta_(mix)V` and `Delta_(mix)H` are zero.

For an ideal solution, Delta_(mix)V is ……….and Delta_(mix)H is ………. .

A: Hexane and heptane forms ideal solution. R: DeltaH,DeltaS and DeltaG are zero for such type of solution.

Assertion (A): Delta_(mix)H and Delta_(mix)V are zero for an ideal solution. Reason (R ): The interactions between the particles of the components of a solution are almost identical as between the particles in liquids.

Delta E and Delta H both are zero in

Enthalpy is an extensive property. In general, if enthalpy of an overall reaction A rarr B along one route is Delta_(r) H " and Delta_(r) H_(1), Delta_(r) H_(2), Delta_(r) H_(3) ..... Represent enthalpies of intermediate reactions leading to product B. What will be the relation between Delta_(r)H overall reaction and Delta_(r)H_(1), Delta_(r)H_(2) ... etc for intermediate reaction.

Assertion:In an ideal solution , Delta_"mix"H is zero Reason :In an ideal solution , A-B interactions are lower than A-A and B-B interactions.

If enthalpy of overall reaction XrarrY along one route is Delta_(r)H and Delta_(r)H_(1),Delta_(r)H_(2),Delta_(r)H_(3) …. Representing enthalpies of reactions leading to same product Y then Delta_(r)H is

Which quantity out of Delta_(r)G " and " Delta_(r) G^(Θ) will be zero at equilibrium ?

How does a non-ideal solution differ from an ideal solution ? When does the positive deviation occur from ideality?

Calculate the enthalpy change when infinitely dilute solution of CaCl_(2) and Na_(2)CO_(3) are mixed. Delta_(f)H^(Theta) for Ca^(2+)(aq), CO_(3)^(2-)(aq) , and CaCO_(3)(s) are -129.80, -161.65 , and -288.50 kcal mol^(-1) respectively.