# The formation of these phosgene is represented as , $CO\ + Cl_2\ \leftrightarrow COCl_2$ . The reaction is carried out in 500 ml flask . At equilibrium 0.3 mole of phosgene , 0.1 mole of CO and 0.1 mole of Cl2 are present. The equlibrium constant of the reaction is : Option 1) 30 Option 2) 15 Option 3) 5 Option 4) 3

As we learned 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

$CO+Cl_{2}\rightleftharpoons COCl_{2}$

At equilibrium  0.1       0.1           0.3

$K=\frac{\left [ COCl_{2} \right ]}{\left [ CO \right ]\left [ Cl_{2} \right ]}$

$=\frac{0.3/0,5}{0.1/0.5\times 0.1/0.5} =\frac{0.5\times0.3}{0.01}=15$

Option 1)

30

Option is incorrect

Option 2)

15

Option is correct

Option 3)

5

Option is incorrect

Option 4)

3

Option is incorrect

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