Which of the following relationship is incorrect
(A) `Delta G^(o)=-2.303RT log k` (B) `Delta G^(o)=-nFE_(cell)^(o)` (C) `Delta H-Delta U=0` (always) (D) `Delta H=Delta U+Delta nRT`

In which of the following Delta H = Delta U ?

For which of the following change Delta H!=Delta U ?

In which of the following changes, Delta H is always negative :

According to the following reaction C(S)+1//2O_(2)(g)rarr CO(g), Delta H=-26.4 Kcal

Complete the following reactions : H_(2)(g)+M_(m)O_(o)(s)overset(Delta)to

The following reactions carried in open vessel. The reaction for which Delta H = Delta U will be

Correct relation for isothermal reversible expansion of an ideal gas is Delta U=0 , Delta S=0 , Delta G=-T Delta S , Delta H=0

Which of the statements are correct about the reaction ? (A) overset(H^(o+))underset(Delta)rarr (B) overset(H_(2)O^(o+))rarr (C ) overset(Delta)rarr (D)

Calculate Delta H^(@)._(f) for chloride ion from the following data : (1)/(2)H_(2)(g) + (1)/(2)Cl_(2)(g) rarr HCI(g), Delta H^(@)._(f) = -92.4 kJ HCI(g) + nH_(2)O rarr H^(+) (aq) + CI^(-)(aq), Delta H^(@) = - 74.8 kJ Delta H^(@)._(f) H^(+) (aq) = 0.0 kJ

For the reaction, A(s) + 3B(g) rarr 4C(g) + d(l) Delta H and Delta U are related as :