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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

`-166.9`

D

`+19.8`

Text Solution

Verified by Experts

The correct Answer is:
D
`DeltaS^(@)=2S_(HCl)^(@)-(S_(H_(2))^(@)+S_(Cl_(2))^(@))`
`=2xx186.7-(130.6+223.0)=19.8 JK^(-1) mol^(-1)`.
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