Home
Class 11
CHEMISTRY
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.

Text Solution

Verified by Experts

The correct Answer is:
10 bar
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • EQUILIBRIUM

    CBSE COMPLEMENTARY MATERIAL|Exercise HOTS QUESTIONS|10 Videos

  • EQUILIBRIUM

    CBSE COMPLEMENTARY MATERIAL|Exercise UNIT TEST|6 Videos

  • EQUILIBRIUM

    CBSE COMPLEMENTARY MATERIAL|Exercise 2- MARK QUESTIONS|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    CBSE COMPLEMENTARY MATERIAL|Exercise UNIT TEST|9 Videos

  • HYDROCARBONS

    CBSE COMPLEMENTARY MATERIAL|Exercise UNIT TEST|16 Videos

Similar Questions

Explore conceptually related problems

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 .

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

    • Similar Questions

    Explore conceptually related problems

    The equilibrium constant K_(p) , for the reaction N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) is 1.6xx10^(-4) at 400^(@)C . What will be the equilibrium constant at 500^(@)C if the heat of reaction in this temperature range is -25.14 kcal?

    The equilibrium constant for the reaction H_(2)(g)+Br_(2) (I) Leftrightarrow 2HBr (g) is K_(p)=4.5 xx 10^(18) atm at 298K . The vapour pressure of liquid Br_(2) at this temperature is 0.28atm. (a) Find K_(p) at 298K for the reaction. H_(2) (g)+Br_(2) (g) Leftrightarrow 2HBr(g) (b) How will be the equilibrium in part (a) be shifted by an increase in the volume of the container if (i) liquid Br_(2) is absent, and (ii) liquid Br_(2) is present.

    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:

    The equilibrium constant K for the reaction 2HI(g) hArr H_(2)(g)+I_(2)(g) at room temperature is 2.85 and that at 698 K is 1.4 xx10^(-2) . This implies

    For the reaction H_(2(g)) + Br_(2(g)) rarr 2HBr_((g)), Delta H=-72.6 KJ . The heat of formation of the HBr is

    Home
    Profile