For a gaseous equilibrium 2 A( g) ⇌2 B( g)+C(g), Kp has a value of 1.8 at 700 K . What is the

step 1 Here in this question we are given with the value of Kp for the given reaction which means 2A ga

For a gaseous equilibrium 2 A( g) ⇌2 B( g)+C(g), Kp has a...

For a gaseous equilibrium $2 \mathrm{~A}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})+\mathrm{C}_{(\mathrm{g})}, \mathrm{K}_{\mathrm{p}}$ has a value of 1.8 at 700 K . What is the value of $\mathrm{K}_{\mathrm{c}}$ for the equilibrium $2 \mathrm{~B}(\mathrm{~g})+\mathrm{C}_{\mathrm{g})} \longleftrightarrow 2 \mathrm{~A}$ at the same pressure? (a) 0.031 (b) $1.3 \times 10^{-3}$ (c) 44.4 (d) 38

For a gaseous equilibrium
$2 \mathrm{~A}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{~B}(\mathrm{~g})+\mathrm{C}_{(\mathrm{g})}, \mathrm{K}_{\mathrm{p}}$ has a value of 1.8 at 700 K . What is the value of $\mathrm{K}_{\mathrm{c}}$ for the equilibrium $2 \mathrm{~B}(\mathrm{~g})+\mathrm{C}_{\mathrm{g})} \longleftrightarrow 2 \mathrm{~A}$ at the same pressure?
(a) 0.031
(b) $1.3 \times 10^{-3}$
(c) 44.4
(d) 38

Key Concepts

Stoichiometric Effects on Equilibrium

The stoichiometric coefficients in a balanced chemical equation impact the change in the number of moles of gas (?n), which in turn affects the equilibrium constant relationship between Kp and Kc. Additionally, reversing a reaction inverts the equilibrium constant, illustrating the importance of reaction direction in equilibrium calculations.

Relationship Between Kp and Kc

Kp and Kc are connected by the equation Kp = Kc(RT)^(?n), where R is the gas constant, T is the temperature in Kelvin, and ?n is the change in the number of moles of gas (moles of gaseous products minus moles of gaseous reactants). This relationship is critical when converting between equilibrium constants expressed in different units, especially for reactions involving gases.

Equilibrium Constants (Kp and Kc)

Equilibrium constants provide a quantitative measure of the concentrations or partial pressures of reactants and products at equilibrium. Kc is defined in terms of molar concentrations, while Kp is defined in terms of partial pressures. These constants are interrelated and provide essential information about the position of equilibrium for a chemical reaction.

Chemical Equilibrium

This concept refers to the state where the rates of the forward and reverse reactions are equal, so that the concentrations (or partial pressures) of the reactants and products remain constant in time. Understanding chemical equilibrium is fundamental in determining how reactions behave under varying conditions and how the equilibrium constant quantifies this balance.

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