I have been stuck on this for the past few hours, and still have got no resolution:
Let's say that we have an isobaric process being done by $1$ mol of a gas. Accordingly, we'll be using gas laws and the first law of thermodynamics to analyze the situation.
So, by the ideal gas law:
$$PV=nRT$$
For sake of understanding, we take $n = 1\space \mathrm {mol}$:
$$\Rightarrow PV=RT \tag{1}$$
Now, using First Law of Thermodynamics,
$$\delta Q = \delta W + \mathrm d U$$ and $\mathrm d U = C_v\, \mathrm d T$, $\space\space\delta W=P\, \mathrm dV$
$$\Rightarrow \delta Q = P\, \mathrm d V + C_v\, \mathrm dT \tag{2}$$
Dividing $(2)$ by $T$, we get,
$$\frac{\delta Q}{T} = \frac{P\, \mathrm dV}{T} + \frac{C_v\, \mathrm d T}{T} \tag{3}$$
Using $(1)$ in $(3)$,
$$\frac{\delta Q}{T} = \frac{R\, \mathrm d V}{V} + \frac{C_v\, \mathrm dT}{T}$$
And $ \displaystyle \frac{\delta Q}{T} = \mathrm dS$,
$$\Rightarrow \mathrm d S = \frac{R\, \mathrm dV}{V} + \frac{C_v\, \mathrm d T}{T} \tag{4}$$
Integrating $(4)$, we get,
$$\Delta S = R\,\ln\left(\frac{V_2}{V_1}\right)+C_v\,\left(\frac{T_2}{T_1}\right)$$
Now, if $T$ decreases in this process, then by the ideal gas law, $V$ should also decrease. If this follows, then the both the terms $R\ln(\frac{V_2}{V_1})$ and $C_v(\frac{T_2}{T_1})$ become negative as $T_2<T_1$ and $V_2<V_1$. So, the overall $RHS$ should become negative, and consequently, $\Delta S$ should become negative.
Please help to point out my mistake in the above mentioned text. Is $\Delta S$ coming negative because I have used an ideal gas?