The equilibrium constant for the H2+(1)/(2) O2 ⇌H2 O reaction at 1 atm and 1200 K is KP · Use th

step 1 Problem number 6. For A, at 1 atmosphere, the chemical reaction is H2 plus half o2 equal to H2O.

The equilibrium constant for the H2+(1)/(2) O2 ⇌H2 O...

The equilibrium constant for the $\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons$ $\mathrm{H}_{2} \mathrm{O}$ reaction at 1 atm and $1200 \mathrm{K}$ is $K_{P \cdot}$ Use this information to determine the equilibrium constant for the following reactions: $(a)$ at 1 atm $\quad \mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}$ $(b)$ at $7 \mathrm{atm} \quad \mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}$ $(c)$ at $1 \mathrm{atm} \quad 3 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons 3 \mathrm{H}_{2}+\frac{3}{2} \mathrm{O}_{2}$ $(d)$ at 12 atm $\quad 3 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons 3 \mathrm{H}_{2}+\frac{3}{2} \mathrm{O}_{2}$

The equilibrium constant for the $\mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons$ $\mathrm{H}_{2} \mathrm{O}$ reaction at 1 atm and $1200 \mathrm{K}$ is $K_{P \cdot}$ Use this information to determine the equilibrium constant for the following reactions:
$(a)$ at 1 atm $\quad \mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}$
$(b)$ at $7 \mathrm{atm} \quad \mathrm{H}_{2}+\frac{1}{2} \mathrm{O}_{2} \rightleftharpoons \mathrm{H}_{2} \mathrm{O}$
$(c)$ at $1 \mathrm{atm} \quad 3 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons 3 \mathrm{H}_{2}+\frac{3}{2} \mathrm{O}_{2}$
$(d)$ at 12 atm $\quad 3 \mathrm{H}_{2} \mathrm{O} \rightleftharpoons 3 \mathrm{H}_{2}+\frac{3}{2} \mathrm{O}_{2}$

Key Concepts

Pressure Effects on Equilibrium in Gas?Phase Reactions

For gas-phase reactions the equilibrium constant expressed in terms of partial pressures (Kp) is defined at a given temperature and is independent of the total pressure. However, adjustment in total pressure changes the partial pressures of the reactants and products, potentially shifting the equilibrium position according to Le Chatelier’s principle. Understanding how changes in total pressure affect the reaction system is crucial for predicting equilibrium behavior under non?standard conditions.

Equilibrium Constant (Kp) Expression

This concept involves writing the equilibrium constant for a reaction in terms of the partial pressures of the gaseous reactants and products. The expression is constructed by raising the partial pressures of each species to the power of their stoichiometric coefficients. It provides a quantitative measure of the position of equilibrium at a given temperature.

Reaction Stoichiometry and Equilibrium Constant Manipulation

When a reaction is reversed or its coefficients are multiplied by a factor, the equilibrium constant is modified accordingly. For example, reversing a reaction inverts the equilibrium constant, and multiplying all coefficients by a factor n raises the equilibrium constant to the nth power. This is essential for determining the new equilibrium constant when the original reaction is altered.

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