Home
Class 11
CHEMISTRY
The value of K(c) for the reaction H(2...

The value of `K_(c)` for the reaction
`H_(2)(g)+I_(2)(g) hArr 2HI(g)`
is `64` at `773K`. If one "mole" of `H_(2)`, one mole of `I_(2)`, and three moles of HI are taken in a `1 L` flask, find the concentrations of `I_(2)` and HI at equilibrium at `773 K`.

Text Solution

AI Generated Solution

To solve the problem step by step, we will follow the process of determining the equilibrium concentrations of the reactants and products based on the initial amounts and the equilibrium constant \( K_c \). ### Step 1: Write the balanced chemical equation The balanced chemical reaction is: \[ \text{H}_2(g) + \text{I}_2(g) \rightleftharpoons 2 \text{HI}(g) \] ### Step 2: Identify the initial concentrations Given: ...
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY ENGLISH|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

The value of K_(c) for the reaction: H_(2)(g)+I_(2)(g) hArr 2HI (g) is 48 at 773 K. If one mole of H_(2) , one mole of I_(2) and three moles of HI are taken in a 1L falsk, find the concentrations of I_(2) and HI at equilibrium at 773 K.

The value of K_(c) for the reaction : H_(2)(g)+I_(2)(g)hArr 2HI(g) is 45.9 at 773 K. If one mole of H_(2) , two mole of I_(2) and three moles of HI are taken in a 1.0 L flask, the concentrations of HI at equilibrium at 773 K.

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

For the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) , the rate of reaction is expressed as

For the reaction 2HI(g)hArr H_(2)(g)+I_(2)(g) . The value of K_(c) is 4. If 2 moles of H_(2)," 2 moles of "I_(2) and 2 moles of HI are present in one litre container then moles of I_(2) present at equilibrium is :

For the equilibrium H_(2)(g)+CO_(2)(g)hArr hArr H_(2)O(g)+CO(g), K_(c)=16 at 1000 K. If 1.0 mole of CO_(2) and 1.0 mole of H_(2) are taken in a l L flask, the final equilibrium concentration of CO at 1000 K will be

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with

For the reaction H_(2)(g)+I_(2)(g) hArr 2HI(g) , the equilibrium can be shifted in favour of product by

One mole of H_(2) two moles of I_(2) and three moles of HI are injected in one litre flask. What will be the concentration of H_(2), I_(2) and HI at equilibrium at 500^(@)C. K_(c ) for reaction H_(2)+I_(2) hArr 2HI is 45.9 .