Question

A mixture containing initially 3.90 mole of NO(g) and 0.88 mole of CO2(g) was allowed to react in a flask of volume 1.00 L at a certain temperature according to the reaction CO2(g) + NO(g) ↔ CO(g) + NO2(g) At equilibrium 0.11 mole of CO2(g) was found present in the reaction mixture. Calculate the equilibrium constant Kc for the reaction at the temperature of the experiment.

Answer 1

Answer:

Equilibrium constant Kc for the reaction will be 1.722

Explanation:

O2(g)+NO(g)→CO(g)+ NO2(g)

0.88    3.9        ---         ---

0.88x   3.9-x     x           x

GIVEN:

0.88X-X= 0.11

⇒ X=0.77

CO2(g)+NO(g) → CO(g) + NO2(g)

0.88       3.9         ---          ---

0.88-x    3.9-x      x            x

=              3.13       0.77      0.77

=0.11

Kc = $\frac{[CO] *[NO2]} {[CO2]*[NO]}$

     =${{0.77}×0.77÷{{0.11×3.13}}$

     = 1.722