For the reversible reaction, N2( g)+3 H2( g) ⇌2 NH3( g) At 500 ^∘ C, the value of Kp is 1.44 ×10

step 1 In this problem, I can calculate the value of DLN which is equal to 2 minus 4 according to the g

For the reversible reaction, N2( g)+3 H2( g) ⇌2 NH3( g) At...

For the reversible reaction, $\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$ At $500{ }^{\circ} \mathrm{C}$, the value of $\mathrm{K}_{\mathrm{p}}$ is $1.44 \times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $\mathrm{K}_c$, with concentration in mole $\mathrm{L}^{-1}$, is (a) $1.44 \times 10^{-5} /(0.082 \times 500)^{-2}$ (b) $1.44 \times 10^{-5} /(8.314 \times 773)^{-2}$ (c) $1.44 \times 10^{-5}(0.082 \times 773)^2$ (d) $1.44 \times 10^{-5} /(0.082 \times 773)^{-2}$

For the reversible reaction,
$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{NH}_3(\mathrm{~g})$
At $500{ }^{\circ} \mathrm{C}$, the value of $\mathrm{K}_{\mathrm{p}}$ is $1.44 \times 10^{-5}$ when partial pressure is measured in atmospheres. The corresponding value of $\mathrm{K}_c$, with concentration in mole $\mathrm{L}^{-1}$, is
(a) $1.44 \times 10^{-5} /(0.082 \times 500)^{-2}$
(b) $1.44 \times 10^{-5} /(8.314 \times 773)^{-2}$
(c) $1.44 \times 10^{-5}(0.082 \times 773)^2$
(d) $1.44 \times 10^{-5} /(0.082 \times 773)^{-2}$

Key Concepts

Ideal Gas Law

The ideal gas law, expressed as PV = nRT, relates pressure, volume, temperature, and the number of moles of gas. In the context of equilibrium constant conversions, the term RT, derived from the ideal gas law, serves as the scaling factor that converts concentration-based measures to pressure-based measures and vice versa.

Equilibrium Constants

Equilibrium constants, such as Kc and Kp, provide a measure of the relative concentrations or partial pressures of reactants and products at chemical equilibrium. They are fundamental to predicting the direction and extent of chemical reactions under given conditions.

Relationship between Kp and Kc

The relationship between the equilibrium constants Kp (based on partial pressures) and Kc (based on molar concentrations) is given by the formula Kp = Kc (RT)^?n, where R is the ideal gas constant, T is the temperature in Kelvin, and ?n represents the difference in moles of gaseous products and reactants. This conversion is crucial for interpreting equilibrium data provided in different units.

Reaction Stoichiometry

Reaction stoichiometry, particularly the change in the number of moles of gaseous species (?n), is important in equilibrium problems because it determines the exponent in the conversion formula between Kp and Kc. A clear understanding of the stoichiometric coefficients allows for accurate calculation of ?n and subsequent conversion between equilibrium constant expressions.

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