Consider the reaction: CO(g)+H2 O(g) ⟹CO2(g)+H2(g) Kp=0.0611 at 2000 K A reaction mixture ini

step 1 In this equilibrium, we're asked to calculate the equilibrium partial pressure of the products,

Consider the reaction: CO(g)+H2 O(g) ⟹CO2(g)+H2(g) ...

Consider the reaction: $$\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \Longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \quad K_{\mathrm{p}}=0.0611\ at \ 2000 \mathrm{K}$$ A reaction mixture initially contains a CO partial pressure of 1344 torr and a $\mathrm{H}_{2} \mathrm{O}$ partial pressure of 1766 torr at 2000 $\mathrm{K}$ . Calculate the equilib- rium partial pressures of each of the products.

Consider the reaction:
$$\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \Longrightarrow \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g) \quad K_{\mathrm{p}}=0.0611\ at \ 2000 \mathrm{K}$$
A reaction mixture initially contains a CO partial pressure of 1344 torr
and a $\mathrm{H}_{2} \mathrm{O}$ partial pressure of 1766 torr at 2000 $\mathrm{K}$ . Calculate the equilib-
rium partial pressures of each of the products.

Key Concepts

Reaction Stoichiometry

Reaction stoichiometry involves the quantitative relationships between reactants and products in a chemical reaction. It is essential for determining how changes in the amounts of one species affect the others, based on the balanced chemical equation. This concept is crucial for setting up the relationships used in the ICE table and solving equilibrium problems.

ICE Table Method

The ICE Table method (Initial, Change, Equilibrium) is a systematic approach used to organize and calculate the concentrations or pressures of species in a reaction at equilibrium. By listing the initial amounts, the changes that occur as the reaction proceeds, and the final equilibrium values, one can set up equations based on the equilibrium constant to solve for unknown variables.

Partial Pressure

Partial pressure is the pressure exerted by a single gas in a mixture of gases. It is an important concept in gas-phase reactions and is used in equilibrium expressions for gaseous systems. Calculating partial pressures allows one to understand how each component contributes to the overall pressure in the system and how the equilibrium position is influenced by them.

Chemical Equilibrium

Chemical equilibrium describes a state in a chemical reaction where the rates of the forward and reverse reactions are equal, resulting in constant concentrations (or pressures) of reactants and products over time. It is a dynamic balance where molecules are continuously reacting, but no net change in composition is observed.

Equilibrium Constant (Kp)

The equilibrium constant in terms of partial pressures (Kp) is a numerical value that expresses the ratio of the product of the partial pressures of the products to that of the reactants, each raised to the power of their stoichiometric coefficients. It is a quantitative measure of the position of equilibrium and is temperature-dependent.

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