Ethanol boils at '78.4^circ C'. The enthalpy of vaporisation of ethanol is '42.4 kJmol^(-1)'. Calculate the entropy of vaporisation of ethanol.

For the melting of ice at '25^circ C' : 'H_2 O(s) rarr H_2 O(l)' the enthalpy of fusion is '6.97 kJmol^(-1)', and entropy of fusion is '25.4 J mol^(-1) K^(-1)'. Calculate the free energy change and predict whether melting of ice is spontaneous or not at this temperature.

The boiling point elevation constant of toluene is 3.32K kg "mol"^(-1) and the normal boiling point of toluene is 110.7^(@)C . The enthalpy of vaporisation of toluene would be nearly

The enthalpy change in a process is the same, whether the process is carried out in a single step or inseveral steps. a) Identify tha law stated here. b) Calculate the enthalpy of formation of CH_4 from the following data : i) C_((s))+O_(2(g))rightarrowCO_(2(g)) DeltaH = -393.7kJ/mol ii) H_(2(g))+frac{1}{2}O_(2(g))rightarrowH_2O_((l)) DeltaH = -285.8kJ/mol iii) CH_(4(g))+2O_(2(g))rightarrowCO_(2(g)) DeltaH =-890.4kJ/mol

The standard enthalpies of combustion of C_(2) H_(5) (g) and ethanol are -393.5, -286 and -1368 kJ respectively. The heat of formation of ethanol is : -277 kJ mol ^(-1) , + 277 kJ mol ^(-1) , - 554 kJ mol ^(-1) , + 554 kJ mol ^(-1)