For the dissociation equilibrium, N_(2)O_(4(g))iff2NO_(2(g)), the variation of free energy with the fraction of N_(2)O_(4) dissociated under standard conditions is shown in the figure : Which of the following statements is/are correct?

For the dissociation equilibrium, N_(2)O_(4(g))iff2NO_(2(g)), the var

1.	For the dissociation equilibrium, N_(2)O_(4(g))iff2NO_(2(g)), the variation of free energy with the fraction of N_(2)O_(4) dissociated under standard conditions is shown in the figure : Which of the following statements is/are correct?
Answer» The free ENERGY CHANGE for the forward reaction is NEGATIVE The free energy change for the backward reaction is negative The NET free energy change for the complete reaction is positive Forward reaction is more SPONTANEOUS than backward reaction Solution :`DeltaG^(@)` for conversion of 1 mole of `N_(2)O_(4)` into equilibrium mixture (forward reaction) `=-0.84kJ,i.e.,-ve` `DeltaG^(@)` for conversion of 1 mole of `N_(2)O_(4)` completely into 2 moles of `NO_(2)=+5.40kJ`. `DeltaG^(@)` for complete conversion is positive therefore, complete conversion is not possible. As `DeltaG^(@)` for backward reaction is more negative than for forward reaction, i.e., formation of `N_(2)O_(4)` is more spontaneous.