In conversion of lime-stone to lime,
`CaCO_(3(s)) to CaO_((s)) + CO_(2(g))` the values of `DeltaH^@` and `DeltaS^@` are `+179.1 kJmol^(-1)` and `160.2 J//K` respectively at `298K` and 1 bar. Assuming that `DeltaH^@` and `DeltaS^@` do not change with temperature, temperature above which conversion of lime-stone to lime will be spontaneous is :

Options

A. `1008 K`
B. `1200 K`
C. `845 K`
D. `1118K`

Answer

d

Explanation

We know, `DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
at equilibrium, `DeltaG^(@)=0`
`DeltaH^(@)=TDeltaS^(@)`
`T=(179.1xx1000)/160.2=1118 K`
So, at temperature above `1118 K`, the reaction will become spontaneous.