Question

For an ideal solution, the correct option is:

• A. \(\Delta_{mix}\) \(S=0 \)at constant \(T\) and \(P \)
• B. \(\Delta_{mix}\) \(V\neq0\)at constant \(T\) and \(P\)
• C. \(\Delta_{mix}\) \(H=0\)at constant \(T\) and \(P\)
• D. \(\Delta_{mix}\) \(G=0\)at constant \(T\) and \(P\)

Answer 1

The Correct Option is C

To solve this question, let's analyze the properties of an ideal solution based on the given options:

1. \(\Delta_{mix}\) \(S = 0\) at constant \(T\) and \(P\):
   In an ideal solution, the entropy of mixing, \(\Delta_{mix} S\), is actually greater than 0. This is because the mixing process increases the randomness of the molecules, resulting in a positive change in entropy.
2. \(\Delta_{mix}\) \(V \neq 0\) at constant \(T\) and \(P\):
   For ideal solutions, the volume of mixing, \(\Delta_{mix} V\), is typically zero. This means there is no change in volume upon mixing, as the intermolecular forces are similar between different components of the solution.
3. \(\Delta_{mix}\) \(H = 0\) at constant \(T\) and \(P\):
   This statement is true for ideal solutions. In an ideal solution, the enthalpy of mixing, \(\Delta_{mix} H\), is zero because the interactions between the molecules in the mixture are similar to those in the pure components. Thus, there is no heat absorbed or evolved.
4. \(\Delta_{mix}\) \(G = 0\) at constant \(T\) and \(P\):
   The Gibbs free energy of mixing, \(\Delta_{mix} G\), is typically negative for mixing processes, as mixing is a spontaneous process. Hence, it cannot be zero under these conditions for an ideal solution.

From this analysis, we conclude that the correct answer is: \(\Delta_{mix}\) \(H = 0\) at constant \(T\) and \(P\).