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For a reversible reaction A hArr B. Find...

For a reversible reaction `A hArr B`. Find `(log_(10)K)/(10)` at `2727^(@)`C temperature
Given
`Delta_(r)H^(0)` = - 54.07 kJ `mol^(-1)`
`Delta_(r)S^(0)` = 10 `JK^(-1)`
R = 8.314 `JK^(-1) mol^(-1)`

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The value of log_(10)K for a reaction A hArr B is (Given: Delta_(f)H_(298K)^(Theta) =- 54.07 kJ mol^(-1) , Delta_(r)S_(298K)^(Theta) =10 JK^(=1) mol^(-1) , and R = 8.314 J K^(-1) mol^(-1)

The value of log_(10)K for a reaction A hArr B is (Given: Delta_(f)H_(298K)^(Theta) =- 54.07 kJ mol^(-1) , Delta_(r)S_(298K)^(Theta) =10 JK^(=1) mol^(-1) , and R = 8.314 J K^(-1) mol^(-1)

The approx value of K for a reaction AhArrB is : Given Delta_(r)H_(298K)^(@)=-54.07KJmol^(-1) , Delta_(r)S_(298K)^(@)=10Jk^(-1)mol^(-1) and R=8.314JK^(-1)mol^(-1) .

The value of log_(10)K for the reaction : A harr B , If Delta H^(@) = - 55.07 kj "mole"^(-1) at 298K. Delta S^(@) = 10 jK^(-1) "mole"^(-1) at 298 K , R = 8.314 jK^(-1) "mole"^(-1)