Calculate the equilibrium constant (Kc) for the reaction below if they are present at equilibriu

step 1 Here I can write the value of case c is equal to nab2 square by an a2 and b2 square multiplicati

Calculate the equilibrium constant (Kc) for the reaction...

Calculate the equilibrium constant $\left(K_{c}\right)$ for the reaction below if they are present at equilibrium $5.0$ mole of $A_{2}, 3$ mole of $B_{2}$ and 2 mole of $A B_{2}$ at $8.21$ atm and $300 \mathrm{~K}$ $$ A_{2}(g)+2 B_{2}(g) \rightleftharpoons 2 A B_{2}(g)+\text { Heat } $$ (a) $1.333$ (b) $2.66$ (c) 20 (d) None of these

Calculate the equilibrium constant $\left(K_{c}\right)$ for the reaction below if they are present at equilibrium $5.0$ mole of $A_{2}, 3$ mole of $B_{2}$ and 2 mole of $A B_{2}$ at $8.21$ atm and $300 \mathrm{~K}$
$$
A_{2}(g)+2 B_{2}(g) \rightleftharpoons 2 A B_{2}(g)+\text { Heat }
$$
(a) $1.333$
(b) $2.66$
(c) 20
(d) None of these

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Key Concepts

Stoichiometry

Stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In the context of equilibrium, stoichiometry is used to correctly formulate the expression for Kc by ensuring that the concentrations are raised to the appropriate coefficients as dictated by the reaction equation.

Ideal Gas Law

The ideal gas law (PV = nRT) provides a relationship between pressure, volume, temperature, and the number of moles for gases. It is essential for converting the given information about moles, pressure, and temperature into concentrations, especially in problems involving gas-phase reactions at equilibrium.

Chemical Equilibrium

Chemical equilibrium is the state in which the forward and reverse reactions occur at the same rate, resulting in constant concentrations of reactants and products over time. This concept underpins the idea that a dynamic balance is established in a chemical system.

Equilibrium Constant (Kc)

The equilibrium constant, Kc, is a numerical expression that relates the concentrations of products and reactants at equilibrium. It is derived from the balanced chemical equation, with each concentration raised to the power of its stoichiometric coefficient, and indicates the extent to which a reaction will proceed under specified conditions.

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