Write the expression for the equilibrium constant Kc for the following

1.	Write the expression for the equilibrium constant Kc for the following reaction: 4 NO(g) + 6H2O (g) ↔ 4 NH3 (g) + 5 O2 (g)
Answer» Law of Mass Action : It was PUT forward by Guldberg and Waag. It states that the rate at which a substance reacts is directly proportional to its active mass and HENCE the rate at which substances react together is directly proportional to the product of their active masses. Active mass means molar concentration. Law of Chemical Equilibrium : For the reaction, $\star\bf\:aA+bB\:\rightleftharpoons\:xX+yY$ Equilibrium constant is given by $\dag\:\underline{\boxed{\bf{\orange{K_c=\dfrac{[X]^x[Y]^y}{[A]^a[B]^b}}}}}$ Where KC is called equilibrium constant at constant temperature. For the given chemical reaction, $\dag\:\underline{\boxed{\bf{\gray{K_c=\dfrac{[NH_3]^4[O_2]^5}{[NO]^4[H_2O]^6}}}}}$ Additional Information : A reaction is said to be in equilibrium when the rate of forward reaction becomes equal to the rate of backward reaction. At equilibrium the concentration of each of the reactants and products becomes constant. A chemical equilibrium can be ESTABLISHED only if none of the products is allowed to escape out.

Write the expression for the equilibrium constant Kc for the following reaction: 4 NO(g) + 6H2O (g) ↔ 4 NH3 (g) + 5 O2 (g)

Answer»

It was PUT forward by Guldberg and Waag.
It states that the rate at which a substance reacts is directly proportional to its active mass and HENCE the rate at which substances react together is directly proportional to the product of their active masses.
Active mass means molar concentration.

For the reaction,

$\star\bf\:aA+bB\:\rightleftharpoons\:xX+yY$

Equilibrium constant is given by

$\dag\:\underline{\boxed{\bf{\orange{K_c=\dfrac{[X]^x[Y]^y}{[A]^a[B]^b}}}}}$

Where KC is called equilibrium constant at constant temperature.

For the given chemical reaction,

$\dag\:\underline{\boxed{\bf{\gray{K_c=\dfrac{[NH_3]^4[O_2]^5}{[NO]^4[H_2O]^6}}}}}$

A reaction is said to be in equilibrium when the rate of forward reaction becomes equal to the rate of backward reaction.
At equilibrium the concentration of each of the reactants and products becomes constant.
A chemical equilibrium can be ESTABLISHED only if none of the products is allowed to escape out.