For the reaction SO2( g)+(1)/(2) O2( g) ⇌SO3( g) if Kp=KC(RT)^x where the symbols have usual mea

step 1 In this problem we have given a reaction in which SO2 gas reacts with half mole of O2 gas reacts

For the reaction SO2( g)+(1)/(2) O2( g) ⇌SO3( g) if...

For the reaction $\mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_3(\mathrm{~g})$ if $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{C}}(\mathrm{RT})^{\mathrm{x}}$ where the symbols have usual meaning then the value of $x$ is: (assuming ideality) [2014] (a) $\frac{1}{2}$ (b) 1 (c) -1 (d) $-\frac{1}{2}$

For the reaction $\mathrm{SO}_2(\mathrm{~g})+\frac{1}{2} \mathrm{O}_2(\mathrm{~g}) \rightleftharpoons \mathrm{SO}_3(\mathrm{~g})$ if $\mathrm{K}_{\mathrm{p}}=\mathrm{K}_{\mathrm{C}}(\mathrm{RT})^{\mathrm{x}}$ where the symbols have usual meaning then the value of $x$ is: (assuming ideality)
[2014]
(a) $\frac{1}{2}$
(b) 1
(c) -1
(d) $-\frac{1}{2}$

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Key Concepts

Stoichiometric Analysis in Gas Phase Reactions

Stoichiometry involves analyzing the coefficients of a balanced chemical equation to determine the change in the number of moles of gaseous species, denoted as ?n. In the context of the relationship between Kp and Kc, ?n is computed as the difference between the sum of the stoichiometric coefficients of gaseous products and reactants. This value determines the exponent of RT in the conversion between Kc and Kp, making it a key component in understanding chemical equilibrium for gases.

Relationship between Kp and Kc

This concept refers to the mathematical relation between the equilibrium constant expressed in terms of partial pressures (Kp) and concentrations (Kc) for gaseous reactions. The relation is given 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 moles of gas between products and reactants. This equation arises from combining the ideal gas law with the definition of the equilibrium constant.

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