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The equilibrium constant for the reactio...

The equilibrium constant for the reaction `H_(2)(g) + Br_(2)(g) hArr 2HBr(g) "at "1024 K " is " 1.6 xx 10^(5)`. Find the equilibrium pressure of all gases if `10.0 `bar of HBr is introduced into a sealed container at 1024K.

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10 bar
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The equilibrium constant for the following reaction is 1.6xx10^(5) at 1024 K H_(2)(g)+Br_(2)(g) hArr 2HBr(g) find the equilibrium pressure of all gases if 10.0 bar of HBr is introduced into a sealed container at 1024 K .

The equilibrium constant for the following reactions is 1.6xx10^(5) at 1024 K , H_(2(g))+Br_(2(g))hArr2HBr_((g)) Find the equilibrium pressure of all gases, if 10.0 bar of HBr is introduced into a sealed container at 1024 K .

The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

The equilibrium constant for the reaction H_(2)+Br_(2)hArr2HBr is 67.8 at 300(@)K . The equilibrium constant for the dissociation of HBr is:

The equilibrium constants for the reaction Br_(2)hArr 2Br at 500 K and 700 K are 1xx10^(-10) and 1xx10^(-5) respectively. The reaction is:

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Knowledge Check

  • The equilibrium constant K_(p) for the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) changes if:

    A
    the total pressure changes
    B
    a catalyst is used
    C
    the amounts of `H_(2) and I_(2)` change
    D
    the temperature changes

  • The equilibrium constant for the reaction H_(2)+Br_(2)hArr2HBr is 67.8 at 300(@)K . The equilibrium constant for the dissociation of HBr is:

    A
    `0.0147`
    B
    `67.80`
    C
    `33.90`
    D
    `8.349`

  • The equilibrium constant value K_(p) for the equilibrium : H_(2) (g) + I_(2) hArr 2 HI (g) changes with

    A
    total pressure
    B
    temperature
    C
    catalyst
    D
    amount of `H_(2) and I_(2)` present