Which of the following statements are correct?

Options

A. For the reaction `CaCO_(3)` (calcite ) `rarr CaCO_(3)` (aragonite) given: `Delta_(f) G_(298)^(@)` (calcite) = -1128.8 kJ/mol, `Delta_(f) G_(298)^(@)` (aragonite) = -1127.75 kJ/mol, then calcite form is more stable at standard conditions
B. For the reaction (1) `C_(("diamond")) + 2H_(2(g)) rarr CH_(4(g)), Delta H_(1)`
(2) `C_(("graphite")) + 4H_((g)) rarr CH_(4(g)), DeltaH_(2)`. Then more heat is evolved in reaction (b)
C. `Delta_(f)H^(0) (I_(2), g) = Delta_("sub") H^(0) (I_(2), s) " at " 25^(@)C`
D. For the exothermic reaction `2Ag_((s)) + 1//2O_(2(g)) rarr 2Ag_(2)O_((s))` at 298K. `Delta H lt Delta U`

Answer

A, B, C, D

Explanation

(a) `Delta G` for calcite `rarr` argonite `gt 0`
`rArr` non spontaneous
(b) `C_(g) rarr C_(d), Delta H gt 0`
`rArr Delta H_(2) - Delta H_(1) gt 0 rArr DeltaH_(2) gt Delta H_(1)`
(c ) `I_(2(s)) rarr I_(2(g)) , Delta H_(f_(l_(2_((g))))) = Delta H_("sub"_(l_(2)))`
(d) `Delta ng lt 0 rArr Delta H lt Delta U`