At 427^@C , for a given change the values of DeltaG and DeltaH are -11,500 J mol^(-1) and -11,300 J mol^(-1) respectively. Calculate the value of DeltaS .
E^@ value for Fe^(3+) 3e^(-) to Fe and Fe^(2+) + 2e^(-) to Fe are -0.036 V and -0.44V respectivley. Calculate E^@ and DeltaG^(0) for the cell potential for the reaction Fe + 2Fe^(3+) rarr 3Fe^(2+) .
Heats of ionisation of acetic acid and ammonium hydroxide are x kJ mol^(-1) and y kJ mol^(-1) . Heat of neutralisation of HCl and NaOH is z kJ mol^(-1) . Calculate the heat when acetic acid is neutralised with ammonium hydroxide. (z-(x+y)kJ mol^(-1))
The driving force DeltaG diminishes to zero on the way to equilibrium, just as in any other spontaneous process. Both DeltaG and the corresponding cell potential (E = (DeltaG)/(nF)) zero when the redox reaction comes to equilibrium. The Nernst equation for the redox process of the cell may be given as : E= E^(@) -(0.059)/( n) log Q The key to the relationship is the standard cell potential E^(@) , derived from the standard free energy change as : E^(@)=-(DeltaG^(@))/(nF) . At equilibrium, the Nernst equation is given as : E^(@) = -(0.059)/(n) log K At equilibrium , when K = 1 the correct relation is
Change in enthalpy and change in internal energy are state functions. The value of DeltaH, DeltaU can be determined by using Kirchoff's equation. Calculate the heat of formation of methane, given that heat of formation of water = -286kJ mol^(-1) , heat of combustion of methane = -890kJ mol^(-1) heat of combustion of carbon = -393.5 kJ mol^(-1)
