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The value of 1og(10) K for a reaction Ah...

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`)

A

5

B

10

C

95

D

100

Text Solution

Verified by Experts

The correct Answer is:
B
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Find the value of log_(10)K for the reaction A Given, Delta_(l)H_(298 K)^(@) = -54.07 kJ "mol"^(-1) Delta_(l)S_(298K)^(@) = 10 JK^(-1) "mol"^(-1) R = 8.314 JK^(-1) "mol"^(-1) 2.303 xx 8.314 xx 298 = 5705

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)

Knowledge Check

  • The value of log_(10) K for a reaction A iff B is (Given : Delta_(r)H_(298K)^(@)=-54.07 kJ mol^(-1) , Delta_(r)S_(298 K)^(@)=10 JK^(-1) mol^(-1) and R=8.314 JK^(-) mol^(-1), 2.303 xx 8.314xx298=5705 )

    A
    5
    B
    10
    C
    95
    D
    100

  • The value of log_(10) K for a reaction A hArr B is ( Given : Delta _(r) H_(298K)^(@)= -54.07kJ mol^(-1),Delta_(r)S_(298K)^(@) = 10J K^(-1)mol^(-1) and R = 8.314 JK^(-1) mol^(-1), 2.303 xx 8.314 xx 298 K = 5705)

    A
    5
    B
    10
    C
    95
    D
    100

  • 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) .

    A
    `10^(+10)`
    B
    `10^(-100)`
    C
    `10^(-10)`
    D
    `10^(+100)`

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    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)

    The value of log_10 K for a reaction A to B is Given: Delta_(r) H_(298 K)^(@) = -54.07 kJ "mol"^(-1) , Delta_(r) S_(298 K)^(@) = 10 JK^(-1) "mol"^(-1) R = 8.314 JK^(-1) "mol"^(-1) 2.303 xx 8.314 xx 298 = 5705

    The values of log_(10)K for a reaction A (Given: DeltaH_(298 K)^(@) = -54.075 kJ mol^(-1), Delta_(t)S_(298 K)^(+) = 10 JK^(-1)mol^(-1) and R = 8.314 JK^(-1)mol^(-1) . 2.303 xx 8.314 xx 298 = 5705)

    The value of log_(10)K for a reaction A to B is (Given DeltaH_(r 298K)^(o) = -54.07 kg mol^(-1) DeltaS_(r 298K)^(o) = -10 kg mol^(-1) and R = 8.314 JK^(-1) mol^(-1), 2.303 xx 8.314 xx 298 = 5705)

    For the reation at 300 K A(g)hArrV(g)+S(g) Delta_(r)H^(@)=-kJ//mol, Delta_(r)S^(@)=-0.1K^(-1).mol^(-1) What is the value of equilibrium constant ?

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