For a given reaction, $∆$H =35.5 kJ mol^-1 and $∆$S = 83.6JK^-1 mol^-1. The reaction is spontaneous at:
(Assume that $∆$H and $∆$S do not vary with temperature)
1. T < 425 K
2. T > 425 K
3. All temperatures
4. T > 298 K

For a given reaction,$∆H = 35.5 KJmo{l}^{-1} and ∆S = 83.6 J{K}^{-1}mo{l}^{-1}$ .The reaction is spontaneous at: (Assume that  $∆H$and  $∆S$ do not vary with temperature)
1. T>425K
2. All temperatures
3. T>298K
4. T<425K

The correct thermodynamic conditions for the spontaneous reaction at all temperatures is

$$\begin{gathered} \left(\mathrm{a}\right) ∆\mathrm{H}>0 \mathrm{and} ∆\mathrm{S}<0 \\ \left(\mathrm{b}\right) ∆\mathrm{H}<0 \mathrm{and} ∆\mathrm{S}>0 \\ \left(\mathrm{c}\right) ∆\mathrm{H}<0 \mathrm{and} ∆\mathrm{S}<0 \\ \left(\mathrm{d}\right) ∆\mathrm{H}<0 \mathrm{and} ∆\mathrm{S}=0 \end{gathered}$$