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The reaction 2A_{\left ( g \right )}+B_{\left ( g \right )}\rightleftharpoons 3C_{\left ( g \right )}+D_{\left ( g \right )} is begun with the concentrations of A and B both at an initial value of 1.00M. When equilibrium is reached, the concentrations of D is measured and found to be 0.25M. The value for the equilibrium constant for this reaction is given by the expression

  • Option 1)

    [\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.75 \right )^{2}\left ( 0.25 \right )]

  • Option 2)

    [\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 1.00 \right )^{2}\left ( 1.00 \right )]

  • Option 3)

    [\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.50 \right )^{2}\left ( 0.75 \right )]

  • Option 4)

    [\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.50 \right )^{2}\left ( 0.25 \right )]

 

Answers (1)

best_answer

As we discussed in concept

Law of Chemical equilibrium -

At a given temperature, the product of concentration of the reaction products raised to the respective stoichiometric coefficient in the balanced chemical equation divided by the product of concentration of the reactants raised to their individual stoichiometric coefficients has a constant value.

- wherein

aA+bB\rightleftharpoons cC+dD


K_{c}=\frac{[C]^{c\:[D]^{d}}}{[A]^{a}\:[B]^{b}}

[A],\:[B],\:[C]\:[D]

are equilibrium concentration

 

                        2A (g)   + B (g)      \rightleftharpoons           3C(g) + D(g)

                                     

Initial                1          1                           0            0

 

At Equilibrium  1-(2x.25) 1-0.25                  3x0.25    0.25

                    = 0.5            = 0.75                 = 0.75

Equilibrium constant K = \frac{[C]^{3}.[D]}{[B][A]^{2}}

K = \frac{(0.75)^{3}\times (0.25)}{(0.75)(0.5)^{2}}


Option 1)

[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.75 \right )^{2}\left ( 0.25 \right )]

This option is incorrect.

Option 2)

[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 1.00 \right )^{2}\left ( 1.00 \right )]

This option is incorrect.

Option 3)

[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.50 \right )^{2}\left ( 0.75 \right )]

This option is correct.

Option 4)

[\left ( 0.75 \right )^{3}\left ( 0.25 \right )]\div [\left ( 0.50 \right )^{2}\left ( 0.25 \right )]

This option is incorrect.

Posted by

divya.saini

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