7. Consider the following equilibrium: 2NOCI(g) = 2NO(g) + Cl2(g) K = 1.56 x 10-5 If 2.00 moles of pure nitrogen monoxide and 3.00 moles of pure chlorine gas are placed in a 2.00-L container, calculate the concentration of Cl2(g) once the reaction has reached equilibrium.
Reversible reactions always depict specified expression for equilibrium constant (K). This constant carried connectivity among equilibrium concentration of all involved reactant-product.
Since it is given that 2.00 moles of NO and 3.00 moles of Cl2 are present in the container initially which reflects that there is no NOCl amount present in the solution.
Thus the reaction will proceed in the reverse direction as shown below.
The equilibrium constant expression is shown below.
Here,
The equilibrium constant is “Kc”.
The formula for the calculation of the concentration/molarity is shown below.
Substitute the known values in the equation (II) to calculate the concentrations.
The concentration of NO:
The concentration of Cl2:
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