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Calculate the equilibrium constant, K fo...

Calculate the equilibrium constant, K for the following reaction at 400K?
`2NOCl_((g))iff2NO_((g))+Cl_(2(g))`
Given that `Delta_(r)H^(0)=80.0KJmol^(-1)` and `Delta_(r)S^(0)=120JK^(-1)mol^(-1)` at 400 K.

Text Solution

AI Generated Solution

To calculate the equilibrium constant \( K \) for the reaction \[ 2 \text{NOCl}_{(g)} \iff 2 \text{NO}_{(g)} + \text{Cl}_{2(g)} \] at 400 K, we will use the Gibbs free energy change (\( \Delta G^\circ \)) and the relationship between \( \Delta G^\circ \) and the equilibrium constant \( K \). ...
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Calculate the equilibrium constant, K for the following reaction at 400 K ? 2NOCl(g) hArr 2NO(g) + Cl_(2)(g) Given that Delta_(r) H^(@) = 80.0 kJ mol^(_1) and Delta_(r)S^(@) =120 J K^(-1) mol^(-1) at 400 K.

What is the equilibrium constant K_(c) for the following reaction at 400K ? 2NOCI(g) hArr 2NO(g) +CI_(2)(g) DeltaH^(Theta) = 77.2 kJ mol^(-1) and DeltaS^(Theta) = 122 J K^(-1) mol^(-1) at 400K .

Knowledge Check

  • What is the equilibrium constant, K for the following reaction at 400 K? 2NOCl(g) iff 2NO(g) + Cl_2(g) Delta H = 77.2 kJ "mol"^(-1) and Delta S = 122 JK^(-1) "mol"^(-1) at 400 K

    A
    `1.95 xx 10^(-4)`
    B
    `7.4 xx 10^(-4)`
    C
    `2.28 xx 10^(-3)`
    D
    `1.48 xx 10^(-5)`

  • What is the equilibrium constant, K for the following reaction at 400 K? 2NOCl (g) hArr 2NO(g)+Cl_(2)(g) DeltaH=77.2" kJ "mol^(-1) and DeltaS=122JK^(-1)mol^(-1) at 400K.

    A
    `-3.708`
    B
    `1.95xx10^(-4)`
    C
    `2.8xx10^(4)`
    D
    `1.67xx10^(-5)`

  • Equilibrium constants (K) for the reaction 2NO(g)+Cl_(2)(g)hArr2NOCl(g) is correctly given by the expression

    A
    `([NOCl]^(2))/([NO]^(2)[Cl_(2)])`
    B
    `([2NOCl])/([2NO][Cl_(2)])`
    C
    `([NO]^(2)+[Cl_(2)])/([NOCl])`
    D
    `([NO]^(2)[Cl_(2)])/([NOCl]^(2))`

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