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The molar entropies of HI(g), H(g) and I...

The molar entropies of HI(g), H(g) and I(g) at 298 K are 206.5, 114.6, and 180.7 J `mol^(-1)K^(-1)` respectively. Using the `DeltaG^(@)` given below, calculate the bond energy of HI.
`HI(g)rarrH(g)+I(g)," "DeltaG^(@)=271.8 kJ`

A

`282.4 kJ "mol"^(-1)`

B

`298.3 kJ "mol"^(-1)`

C

`290.1 kJ "mol"^(-1)`

D

`315.4 kJ "mol"^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaS^(@) =-206.5+114.6 +180.7 =88.8`
`DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
`DeltaH^(@)=271.8 + 298 xx88.8 xx 10^(-3)`
`DeltaH^(@)=298.3`
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