For the reaction Cls+CO2( g) ⇌2 CO(g), the partial pressures of CO2 and CO are 4 and 8 atm respe

step 1 In this problem, we have given a reaction in which carbon solid reacts with carbon dioxide gas r

For the reaction Cls+CO2( g) ⇌2 CO(g), the partial pressures...

For the reaction $\mathrm{C}_{\mathrm{ls}}+\mathrm{CO}_2(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})$, the partial pressures of $\mathrm{CO}_2$ and CO are 4 and 8 atm respectively. The value of $\mathrm{K}_{\mathrm{p}}$ for this reaction is (a) 14 atm (b) 16 atm (c) 18 atm (d) 12 atm

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Key Concepts

Partial Pressures

Partial pressures refer to the pressure exerted by individual gases in a mixture. In reactions involving gases, they serve as a measure of the concentration of each species, and are used in the calculation of the equilibrium constant Kp.

Equilibrium Expressions

Equilibrium expressions are mathematical formulations derived from balanced chemical equations that relate the concentrations or partial pressures of reactants and products at equilibrium. They are central to analyzing the state of a system and predicting how changes in conditions affect equilibrium.

Reaction Stoichiometry

Reaction stoichiometry involves the coefficients in the balanced chemical equation. These coefficients indicate the molar ratios in which reactants and products participate in the reaction and determine the exponents in the expression for the equilibrium constant.

Equilibrium Constant (Kp)

The equilibrium constant Kp is a dimensionless value for reactions involving gases. It is defined as the ratio of the product of the partial pressures of the products, each raised to the power of their respective coefficients, to the product of the partial pressures of the reactants, each also raised to the power of their coefficients.

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