369416 Assertion :
Salt such as \(\mathrm{NaCl}\) dissolves, the \(\mathrm{Na}^{+}\)and \(\mathrm{Cl}^{-}\)ions leaving the crystal lattice acquire far greater freedom.
Reason :
In thermodyanamic terms, the formation of solution occurs with a favourable change in free energy, i.e., \(\Delta \mathrm{H}\) has high positive value and \({\text{T}}\Delta {\text{S}}\) has a low negative value.

369417 Assertion :
Heat absorbed in a reaction at constant temperature and constant volume is \(-\Delta \mathrm{G}\).
Reason :
\(\Delta \mathrm{G}\) should be negative for the reaction to be spontaneous.

369418 Which of the following is not correct?

369419 For a reaction \(\mathrm{\mathrm{R}_{1}, \Delta \mathrm{G}=\mathrm{xkJ} \mathrm{mol}^{-1}}\). For a reaction \(\mathrm{\mathrm{R}_{2}, \Delta \mathrm{G}=\mathrm{y} \mathrm{kJ} \mathrm{mol}^{-1}}\). Reaction \(\mathrm{\mathrm{R}_{1}}\) is nonspontaneous but along with \(\mathrm{\mathrm{R}_{2}}\) it is spontaneous. This means that

369416 Assertion :
Salt such as \(\mathrm{NaCl}\) dissolves, the \(\mathrm{Na}^{+}\)and \(\mathrm{Cl}^{-}\)ions leaving the crystal lattice acquire far greater freedom.
Reason :
In thermodyanamic terms, the formation of solution occurs with a favourable change in free energy, i.e., \(\Delta \mathrm{H}\) has high positive value and \({\text{T}}\Delta {\text{S}}\) has a low negative value.

369417 Assertion :
Heat absorbed in a reaction at constant temperature and constant volume is \(-\Delta \mathrm{G}\).
Reason :
\(\Delta \mathrm{G}\) should be negative for the reaction to be spontaneous.

369418 Which of the following is not correct?

369419 For a reaction \(\mathrm{\mathrm{R}_{1}, \Delta \mathrm{G}=\mathrm{xkJ} \mathrm{mol}^{-1}}\). For a reaction \(\mathrm{\mathrm{R}_{2}, \Delta \mathrm{G}=\mathrm{y} \mathrm{kJ} \mathrm{mol}^{-1}}\). Reaction \(\mathrm{\mathrm{R}_{1}}\) is nonspontaneous but along with \(\mathrm{\mathrm{R}_{2}}\) it is spontaneous. This means that

369416 Assertion :
Salt such as \(\mathrm{NaCl}\) dissolves, the \(\mathrm{Na}^{+}\)and \(\mathrm{Cl}^{-}\)ions leaving the crystal lattice acquire far greater freedom.
Reason :
In thermodyanamic terms, the formation of solution occurs with a favourable change in free energy, i.e., \(\Delta \mathrm{H}\) has high positive value and \({\text{T}}\Delta {\text{S}}\) has a low negative value.

369417 Assertion :
Heat absorbed in a reaction at constant temperature and constant volume is \(-\Delta \mathrm{G}\).
Reason :
\(\Delta \mathrm{G}\) should be negative for the reaction to be spontaneous.

369418 Which of the following is not correct?

369419 For a reaction \(\mathrm{\mathrm{R}_{1}, \Delta \mathrm{G}=\mathrm{xkJ} \mathrm{mol}^{-1}}\). For a reaction \(\mathrm{\mathrm{R}_{2}, \Delta \mathrm{G}=\mathrm{y} \mathrm{kJ} \mathrm{mol}^{-1}}\). Reaction \(\mathrm{\mathrm{R}_{1}}\) is nonspontaneous but along with \(\mathrm{\mathrm{R}_{2}}\) it is spontaneous. This means that

369416 Assertion :
Salt such as \(\mathrm{NaCl}\) dissolves, the \(\mathrm{Na}^{+}\)and \(\mathrm{Cl}^{-}\)ions leaving the crystal lattice acquire far greater freedom.
Reason :
In thermodyanamic terms, the formation of solution occurs with a favourable change in free energy, i.e., \(\Delta \mathrm{H}\) has high positive value and \({\text{T}}\Delta {\text{S}}\) has a low negative value.

369417 Assertion :
Heat absorbed in a reaction at constant temperature and constant volume is \(-\Delta \mathrm{G}\).
Reason :
\(\Delta \mathrm{G}\) should be negative for the reaction to be spontaneous.

369418 Which of the following is not correct?

369419 For a reaction \(\mathrm{\mathrm{R}_{1}, \Delta \mathrm{G}=\mathrm{xkJ} \mathrm{mol}^{-1}}\). For a reaction \(\mathrm{\mathrm{R}_{2}, \Delta \mathrm{G}=\mathrm{y} \mathrm{kJ} \mathrm{mol}^{-1}}\). Reaction \(\mathrm{\mathrm{R}_{1}}\) is nonspontaneous but along with \(\mathrm{\mathrm{R}_{2}}\) it is spontaneous. This means that