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Given the following entropy values (in J...

Given the following entropy values (in `JK^(-1)"mol"^(-1))` at 298 K atm : `H_(2)(g):130.6.Cl_(2)(g):223.0andHCl(g): 186.7` . The entropy change (in `JK^(-1)"mol"^(-1))` for the reaction
`H_(2)(g)+Cl_(2)(g)to2HCl(g)`is

A

`+540.3`

B

`+727.3`

C

`-16.69`

D

`+9.9`

Text Solution

Verified by Experts

The correct Answer is:
D
`Delta S_("reaction")=[ Sigma S_("products")^(0)-Sigma S_("reactants")^(0)]`
`=186.7 -[(1)/(2) (130.61)+(1)/(2)(223)]`
`=186.7- [65.305 + 111.5]`
`=186.7-176.805`
`=9.895 = 9.9 J K^(-1) mol^(-1)`
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