Determine the value of kc for the following reaction if the equilibrium concentrations are as follows:
[n2]eq = 1.5 m,[h2]eq = 1.1 m,[nh3]eq = 0.47 m.
n2(g) + 3 h2(g) ⇌ 2 nh3(g)

0.11

Explanation:

The given equilibrium reaction and the equilibrium concentrations are shown below as:-

The Kc of an equilibrium reaction measures relative amounts of the products and the reactants present during the equilibrium.

It is the ratio of the concentration of the products and the reactants each raised to their stoichiometric coefficients. The concentration of the liquid and the gaseous species does not change and thus is not written in the expression.

The equation is as follows:-

The expression for the Kc is:-

Thus, applying the values as:-

in the given question, the partial pressure is calculated by using the ideal gas equation, that is, pv = nrt

here, p is pressure, v is volume = 25 l, n is number of moles = 0.0104 moles, r is gas constant = -0.0821 l.atm / mol.k

t is temperature = 273 k

p = nrt / v

p = (0.0104 mol × 0.0821 l.atm / mol.k × 273 k) / 25 l

= 0.0093 atm