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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 ………

Text Solution

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`K_(p)=K_(c )(RT)^(Deltan)`
`Deltan=`number of moles of gaseous products numbers of moles of gesous reactants
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Knowledge Check

  • STATEMENT-1: For a given reaction at fixed temperatures, equlibrium constants K_(rho)and K_(c) are realated as K_(rho)=K_(c)(RT)^(Deltan) STATEMENT-2: Deltan=No. of moles of product - No of moles of reactants.

    A
    Statement-1 is True, Statement-2 is True, Statement-2 is a correct explanation for Statement-1
    B
    Statement-1 is True, Statement-2 is True, Statement-2 is NOT a correct explanation for Statement-1
    C
    Statement-1 is True, Statement-2 is False
    D
    Statement-1 is False, Statement-2 is True

  • The relation between equilibrium constant K_(p) and K_(c) is

    A
    `K_(c)=K_(p)(RT)^(Deltan)`
    B
    `K_(p)=K_(c)(RT)^(Deltan)`
    C
    `K_(p)=((K_(c))/(RT))^(Deltan)`
    D
    `K_(p)=K_(c)=(RT)^(Deltan)`

  • For a reversible reaction A + B iff C + D the equilibrium constant, K_(C) is equal to

    A
    `([A][B])/([C][D])`
    B
    `([C][D])/([A][B])`
    C
    `([A][C])/([B][D])`
    D
    None of these

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    The relationship between equilibrium constants K_(p) "and" K_(c) for a gaseous reaction is:

    Assertion : The equilibrium constant is fixed and characteristics for any given chemical reaction at a specified temperature. Reason : The equilibrium constant for an exothermic reaction decreases as the temperature increases.

    For a chemical reaction 2A+BiffC , the thermodynamic equilibrium constant K_(p) is

    For a given exthermic reaction , K_(p) nd K_(p) are the equilibrium constants at temperature T_(1) and T_(2) respectively . Assumbing that heat of reaction is constant in temperature range between T_(1) and T_(2) it is readily observed that

    For which of the reversible reaction K_p=K_c

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