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At equilibrium, the rate of forward and ...

At equilibrium, the rate of forward and backward reaction become equal and as a result concentration of each reactant and product becomes constant. The expression and numerical value of equilibrium constant depends upon the form of balanced chemical equation. If stoichiometry of the balanced chemical equation changes, the value of equilibrium constant changes. An equilibrium system for the reaction:
`N_2O_4(g) hArr 2NO_2(g)` at 390 K.
in a 5L flask contains 1.0 mol of `NO_2` and 0.125 mol of `N_2O_4`.
Calculate the value of `K_c` for the above reaction.

Text Solution

AI Generated Solution

To calculate the equilibrium constant \( K_c \) for the reaction \[ N_2O_4(g) \rightleftharpoons 2NO_2(g) \] at 390 K, we will follow these steps: ...
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At equilibrium, the rate of forward and backward reaction become equal and as a result concentration of each reactant and product becomes constant. The expression and numerical value of equilibrium constant depends upon the form of balanced chemical equation. If stoichiometry of the balanced chemical equation changes, the value of equilibrium constant changes. An equilibrium system for the reaction: N_2O_4(g) hArr 2NO_2(g) at 390 K. in a 5L flask contains 1.0 mol of NO_2 and 0.125 mol of N_2O_4 . What is the value of K_p for the reaction?

At equilibrium, the rate of forward and backward reaction become equal and as a result concentration of each reactant and product becomes constant. The expression and numerical value of equilibrium constant depends upon the form of balanced chemical equation. If stoichiometry of the balanced chemical equation changes, the value of equilibrium constant changes. An equilibrium system for the reaction: N_2O_4(g) hArr 2NO_2(g) at 390 K. in a 5L flask contains 1.0 mol of NO_2 and 0.125 mol of N_2O_4 . What will be the value of K_c for the reaction: 1/2N_2O_4(g) hArr NO_2(g)

Knowledge Check

  • The numerical value of the equilibrium constant or any chemical change is affected by changing the

    A
    concentration of product
    B
    catalyst
    C
    concentration of reacting substance
    D
    temperature

  • The numerical value of the equilibrium constant or any chemical change is affected by changing the

    A
    concentration of product
    B
    catalyst
    C
    concentration of reacting substance
    D
    temperature

  • 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

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    At equilibrium, the rate of forward and backward reaction become equal and as a result concentration of each reactant and product becomes constant. The expression and numerical value of equilibrium constant depends upon the form of balanced chemical equation. If stoichiometry of the balanced chemical equation changes, the value of equilibrium constant changes. An equilibrium system for the reaction: N_2O_4(g) hArr 2NO_2(g) at 390 K. in a 5L flask contains 1.0 mol of NO_2 and 0.125 mol of N_2O_4 . What will be the effect on the value of K_c if more of N_2O_4 is added at equilibrium ?

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