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

The question asks about the characteristics of an ideal solution and provides several options regarding mixing properties such as entropy, volume, enthalpy, and Gibbs energy. Let's break down each of the options:

• \(\Delta_{mix}\) \(S=0\) at constant \(T\) and \(P\):

  This statement implies that the change in entropy during the mixing of components is zero. For an ideal solution, the mixing of different components typically leads to an increase in disorder and, consequently, an increase in entropy. Thus, this option is incorrect for ideal solutions.

• \(\Delta_{mix}\) \(V\neq0\) at constant \(T\) and \(P\):

  This statement suggests that there is a change in volume during mixing. However, for an ideal solution, the volume of mixing is assumed to be zero, meaning no unexpected expansion or contraction occurs. Therefore, this option is also incorrect.

• \(\Delta_{mix}\) \(H=0\) at constant \(T\) and \(P\):

  This option states that there is no enthalpy change during mixing. This is a characteristic of ideal solutions, where interactions between the molecules are equal in the pure components and the solution. Hence, this option is correct.

• \(\Delta_{mix}\) \(G=0\) at constant \(T\) and \(P\):

  The Gibbs energy change during mixing for an ideal solution is not zero. In fact, it is negative due to increased entropy, which implies spontaneous mixing. Therefore, this option is incorrect.

In conclusion, for an ideal solution, the correct statement is that the enthalpy change during mixing is zero, i.e., \(\Delta_{mix}\) \(H=0\) at constant \(T\) and \(P\).