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

step 1 So for a reaction that is C plus CO2 gives 2 COO the partial pressure of CO2 and CO1 partial pre

For the reaction C(s)+CO2( g) ⇌2 CO(g) the partial pressurc...

For the reaction $\mathrm{C}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})$ the partial pressurc of $\mathrm{CO}_{2}$ and $\mathrm{CO}$ are 4 and 8 atm, respectively, then $\mathrm{K}_{\mathrm{p}}$ for the reaction is (1) $16 \mathrm{~atm}$ (2) $2 \mathrm{~atm}$ (3) $5 \mathrm{~atm}$ (4) $4 \mathrm{~atm}$

For the reaction $\mathrm{C}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{~g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g})$ the
partial pressurc of $\mathrm{CO}_{2}$ and $\mathrm{CO}$ are 4 and 8 atm, respectively, then $\mathrm{K}_{\mathrm{p}}$ for the reaction is
(1) $16 \mathrm{~atm}$
(2) $2 \mathrm{~atm}$
(3) $5 \mathrm{~atm}$
(4) $4 \mathrm{~atm}$

Key Concepts

Stoichiometry in Equilibrium Expressions

The stoichiometric coefficients from the balanced chemical equation determine the exponents in the equilibrium expression. These coefficients ensure that the contribution of each species to the overall equilibrium is appropriately scaled according to the reaction's balanced law, leading to an accurate representation of the reaction's equilibrium state.

Equilibrium Constant (Kp)

Kp is the equilibrium constant defined in terms of the partial pressures of gaseous reactants and products. It is calculated by taking the product of the partial pressures of the products (each raised to the power of their stoichiometric coefficients) and dividing it by the product of the partial pressures of the reactants (also raised to the power of their stoichiometric coefficients). This constant provides an understanding of the relative concentrations of species at equilibrium under a given set of conditions.

Partial Pressure

Partial pressure is the pressure that an individual gas exerts within a mixture of gases. It is used in equilibrium expressions for gaseous reactions to represent the effective concentration of each species, thereby allowing chemists to relate the pressure conditions to the position of equilibrium.

Activity of Pure Solids

In equilibrium calculations, the activity of a pure solid is considered to be unity because its concentration remains constant regardless of changes in the system. This simplification means that pure solids are omitted from the equilibrium constant expression, focusing the calculation solely on the gaseous or dissolved species.

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