In conversion of lime-stone to lime, CaCO3(s)⟶CaO(s)+CO2(g) he values of ΔH∘ and ΔS∘ are 179.1kJmol-1 and 160.2JK−1mol−1 respectively at 298 K and 1 bar. Assuming that  ΔH∘and ΔS∘do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

# In conversion of lime-stone to lime, ${\mathrm{CaCO}}_{3}\left(\mathrm{s}\right)⟶\mathrm{CaO}\left(\mathrm{s}\right)+{\mathrm{CO}}_{2}\left(\mathrm{g}\right)$ he values of $\mathrm{\Delta }{H}^{\circ }$ and $\mathrm{\Delta }{S}^{\circ }$ are $179.1{\mathrm{kJmol}}^{-1}$ and $160.2{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$ respectively at 298 K and 1 bar. Assuming that  $\mathrm{\Delta }{H}^{\circ }$and $\mathrm{\Delta }{S}^{\circ }$do not change with temperature, temperature above which conversion of limestone to lime will be spontaneous is

1. A

2. B

3. C

4. D

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### Solution:

The temperature at which given reaction exists as equilibrium is

At $T>{T}_{\mathrm{eq}},\mathrm{\Delta }{G}^{\circ }$of the reaction will be negative and hence the given reaction will be spontaneous.

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