List of top Chemistry Questions on Gibbs energy change and equilibrium

Which of the following statements are incorrect for thermodynamic properties? (A) Both \(E_{\text{cell}}\) and \(\Delta_r G\) of reaction are extensive properties. (B) Both \(E_{\text{cell}}\) and \(\Delta_r G\) of reaction are intensive properties. (C) \(E_{\text{cell}}\) is an intensive property while \(\Delta_r G\) of reaction is an extensive property. (D) \(E_{\text{cell}}\) is an extensive property while \(\Delta_r G\) of reaction is an intensive property. Choose the answer from the options given below:

At the state of dynamic equilibrium, for solute + solvent gives solution.

At the state of dynamic equilibrium, for solute + solvent gives solution.

At the state of dynamic equilibrium, for solute + solvent gives solution.

At the state of dynamic equilibrium, for solute + solvent gives solution.

For a reaction taking place in four different steps, the rate constants follow a relationship \(K-\frac{K_2K_4}{K_1K_3}\). If the energies of activation E₁, E₂, E₃ and E₄ are 10 kJ/mol, 30kJ/mol, 40 kJ/mol and 20 kJ/mol respectively, then the overall energy of activation would be :

For the reaction at \(298\ K\),
\(2A+B→C\)
\(∆H = 400\ kJ mol^{-1}\) and \(∆S = 0.2\ kJ K^{-1} mol^{-1}\)
At what temperature will the reaction become spontaneous considering \(∆H\) and \(∆S\) to be constant over the temperature range.

For the reaction, \(2Cl(g)→Cl_2(g)\), what are the signs of \(∆H\) and \(∆S\) ?

For the reaction
\(2A(g)+B(g)→2D(g)\)
\(∆U^Θ= -10.5\ kJ\) and \(∆S^Θ= -44.1\ JK^{-1}\).
Calculate \(∆G^Θ\) for the reaction, and predict whether the reaction may occur spontaneously.