The entropy change of an ideal gas closed system is a function of only temperature

The statement is partially correct. The entropy change of an ideal gas in a closed system is indeed a function of temperature, but it also depends on other factors.

Entropy (S) is a thermodynamic property that is a measure of a system's thermal energy per unit temperature that is unavailable for doing useful work. For an ideal gas, the change in entropy (ΔS) can be calculated using the formula:

ΔS = nRln(T2/T1) + nCln(V2/V1)

where:

• n is the number of moles of the gas,
• R is the universal gas constant,
• T1 and T2 are the initial and final temperatures,
• C is the molar heat capacity at constant pressure,
• V1 and V2 are the initial and final volumes.

From this equation, we can see that the entropy change depends not only on the initial and final temperatures, but also on the initial and final volumes of the gas, the number of moles of the gas, and the molar heat capacity at constant pressure. Therefore, while temperature is a key factor, it is not the only factor that determines the entropy change of an ideal gas in a closed system.