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For a given reversible reaction at a fix...

For a given reversible reaction at a fixed temperature, equilibrium constants `K_(p)` and `K_(c)` are related by ………

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To derive the relationship between the equilibrium constants \( K_p \) and \( K_c \) for a given reversible reaction at a fixed temperature, we can follow these steps: ### Step 1: Understand the Definitions - **Equilibrium Constant \( K_c \)**: This is the equilibrium constant expressed in terms of molarity (concentration) of the reactants and products. - **Equilibrium Constant \( K_p \)**: This is the equilibrium constant expressed in terms of partial pressures of the reactants and products. ### Step 2: Write the General Reaction Consider a general reversible reaction: ...
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For a gaseous reaction 2B rarr A , the equilibrium constant K_(p) is ……… to // than K_(c) .

For a reversible reaction at 298 K the equilibrium constant K is 200. What is value of DeltaG^(@) at 298 K ?

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Knowledge Check

  • For a reversible reaction at 298 K the equilibrium constant K is 200. What is value of DeltaG^(@) at 298 K ?

    A
    a. `-13.13kcal`
    B
    b.-0.13kcal`
    C
    c. `-3.158kcal`
    D
    d. `-0.413kcal`

  • For a given exothermic reaction , K_P and K_p' are the equilibrium constant at temperature T_1 and T_2 respectively .Assuming that heat of reaction is constant in temperature range between T_1 and T_2 , it is readly observed that

    A
    ` K_p gt K_p `
    B
    ` K_p lt K_p `
    C
    ` K_p = K_p `
    D
    ` K_p = (1)/(K_p')`

  • The equilibrium constant of a reversible reaction at a given temperature

    A
    depends on initial concentration of reactants
    B
    depends on the concentration of products at equilibrium
    C
    does not depend on the initial concentration
    D
    is not a characteristic of the reaction.