For the reaction, [2005] 2 NO2( g) ⇄2 NO( g)+O2( g) (Kc=1.8 ×10^-6 at 184^∘ C)

step 1 As we know that as we know that the formula for KP is equal to KC RT to the power DL N. Here the

For the reaction, [2005] 2 NO2( g) ⇄2 NO( g)+O2( g) ...

For the reaction, [2005] $$ \begin{aligned} & 2 \mathrm{NO}_2(\mathrm{~g}) \rightleftarrows 2 \mathrm{NO}(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \\ & \left(\mathrm{K}_{\mathrm{c}}=1.8 \times 10^{-6} \text { at } 184^{\circ} \mathrm{C}\right) \\ & (\mathrm{R}=0.0831 \mathrm{~kJ} /(\mathrm{mol} \mathrm{~K})) \end{aligned} $$ when $\mathrm{K}_{\mathrm{p}}$ and $\mathrm{K}_{\mathrm{c}}$ are compared at $184^{\circ} \mathrm{C}$ it is found that (a) $\mathrm{K}_{\mathrm{p}}$ is greater than $\mathrm{K}_{\mathrm{c}}$ (b) $\mathrm{K}_{\mathrm{p}}$ is less than $\mathrm{K}_{\mathrm{c}}$ (c) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{e}}$ (d) whether $\mathrm{K}_{\mathrm{p}}$ is greater than, less than or equal to $\mathrm{K}_{\mathrm{c}}$ depends upon the total gas pressure

For the reaction,
[2005]

$$
\begin{aligned}
& 2 \mathrm{NO}_2(\mathrm{~g}) \rightleftarrows 2 \mathrm{NO}(\mathrm{~g})+\mathrm{O}_2(\mathrm{~g}) \\
& \left(\mathrm{K}_{\mathrm{c}}=1.8 \times 10^{-6} \text { at } 184^{\circ} \mathrm{C}\right) \\
& (\mathrm{R}=0.0831 \mathrm{~kJ} /(\mathrm{mol} \mathrm{~K}))
\end{aligned}
$$

when $\mathrm{K}_{\mathrm{p}}$ and $\mathrm{K}_{\mathrm{c}}$ are compared at $184^{\circ} \mathrm{C}$ it is found that
(a) $\mathrm{K}_{\mathrm{p}}$ is greater than $\mathrm{K}_{\mathrm{c}}$
(b) $\mathrm{K}_{\mathrm{p}}$ is less than $\mathrm{K}_{\mathrm{c}}$
(c) $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{e}}$
(d) whether $\mathrm{K}_{\mathrm{p}}$ is greater than, less than or equal to $\mathrm{K}_{\mathrm{c}}$ depends upon the total gas pressure

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Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in which the forward and reverse reactions occur at equal rates in a reversible process, leading to constant concentrations or partial pressures of reactants and products. This equilibrium is characterized by an equilibrium constant that quantifies the ratio of products to reactants at equilibrium.

Equilibrium Constants for Gases (Kc and Kp)

For gaseous reactions, equilibrium can be expressed in terms of concentrations (Kc) or partial pressures (Kp). These two constants are interrelated 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 between products and reactants.

Reaction Stoichiometry and Change in Moles (?n)

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. In gas-phase equilibria, the term ?n is defined as the difference between the sum of moles of gaseous products and the sum of moles of gaseous reactants. This change in mole number is critical when converting between Kc and Kp, as it determines whether the equilibrium constant based on partial pressures will be larger or smaller than that based on concentrations.

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