Calculate the enthalpy change on freezing of '1.0 mol' of water at '10.0^circ C' to ice at '-10.0^circ C . Delta_( fus) H=6.03 kJ mol^(-1)' at '0^circ C .'
'C_p[H_2 O(t)]=7 5 . 3 J m o l^(-1) K^(-1)'
'C_p[H_2 O(s)]=36.8 J mol^(-1) K^(-1)'

Calculate the entropy change in surrounding when 1.0 mol of H_2O(l) is formed under standard conditions. Given Delta_fH^o = -286 kJ mol^-1.

The enthalpy change for the conversion of liquid water to steat is '40.8 k J' at '100^circ C'. Calculate 'Delta S' for the process.

The enthalpy change in freezing 1 g of water (Delta _fusion H = 6 .0 kJ mol^(-1) ) will be:- -6000.0 J , -333 J , 333.33J , 60.0 J

Calculate the enthalpy change for the process 'CCl_4(g) rarr C(g)+4 Cl(g)' and calculate bond enthalpy of 'C-Cl' in 'CCl_4(g)' 'Delta_(vap) H_^0 (C C l_4)=30.5 kJ mol ^(-1)' 'Delta_f H^0(C C l_4)=(-1)35.5 kJ mol^(-1)' 'Delta_n H^0(C)=715.0 kJ mol^(-1)', where 'Delta_n H^0' is enthalpy of atomisation, 'Delta_n H^ (Cl_2)=242 kJ mol^(-1)'