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The value of log(10)K for a reaction A h...

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)`

A

5

B

10

C

95

D

100

Text Solution

Verified by Experts

The correct Answer is:
B
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The value of 1og_(10) K for a reaction AhArrB is: (Given, Delta_(r)H_(298K)^(@)=-54.07kJ" "mol^(-1),Delta_(r)S_(298K)^(@)=10JK^(-1)" "mol^(-1) and R=8.314JK^(-1)" "mol^(-1),2.303xx8.314xx298=5705 )

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) .

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)

Calculate the standard free energy change for the reaction: H_(2)(g) +I_(2)(g) rarr 2HI(g), DeltaH^(Theta) = 51.9 kJ mol^(-1) Given: S^(Theta) (H_(2)) = 130.6 J K^(-1) mol^(-1) , S^(Theta) (I_(2)) = 116.7 J K^(-1) mol^(-1) and S^(Theta) (HI) =- 206.8 J K^(-1) mol^(-1) .

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