In the reaction BaO2( s) ⟺BaO(s)+O2( g); ΔH=+ ve. In equilibrium condition, pressure of O2 depen

step 1 In this problem, we have given a reaction, barium oxide reacts reversibly and give barium oxide

In the reaction BaO2( s) ⟺BaO(s)+O2( g); ΔH=+ ve. In...

In the reaction $\mathrm{BaO}_2(\mathrm{~s}) \Longleftrightarrow \mathrm{BaO}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g})$; $\Delta \mathrm{H}=+$ ve. In equilibrium condition, pressure of $\mathrm{O}_2$ depends on (a) increase mass of $\mathrm{BaO}_2$ (b) increase mass of BaO (c) temperature of equilibrium (d) mass of $\mathrm{BaO}_2$ and BaO both

In the reaction $\mathrm{BaO}_2(\mathrm{~s}) \Longleftrightarrow \mathrm{BaO}(\mathrm{s})+\mathrm{O}_2(\mathrm{~g})$; $\Delta \mathrm{H}=+$ ve. In equilibrium condition, pressure of $\mathrm{O}_2$ depends on
(a) increase mass of $\mathrm{BaO}_2$
(b) increase mass of BaO
(c) temperature of equilibrium
(d) mass of $\mathrm{BaO}_2$ and BaO both

Key Concepts

Chemical Equilibrium

Chemical equilibrium refers to the state in a reversible reaction where the rates of the forward and reverse reactions are equal. At this point, the concentrations (or pressures, for gases) of reactants and products remain constant over time. Understanding chemical equilibrium involves recognizing that the system's conditions determine the final concentrations based on the equilibrium constant, not solely on the amounts of substances initially present.

Heterogeneous Equilibrium

Heterogeneous equilibrium occurs when the reaction involves more than one phase, such as solids and gases. In such systems, the activities of pure solids (and pure liquids) are taken as constant (typically unity) and do not appear in the expression for the equilibrium constant. This means that changes in the amount of solid reactants or products do not affect the equilibrium position, as their effective concentrations are fixed by their phase.

Equilibrium Constant and Its Dependence on Temperature

The equilibrium constant (K) for a reaction quantifies the ratio of products to reactants at equilibrium. For heterogeneous reactions, this constant typically involves only the gaseous or aqueous components. The value of K is dependent solely on temperature; for an endothermic reaction, an increase in temperature leads to an increase in K. Therefore, in such systems, variables like pressure or concentration of the gas phase are directly influenced by temperature changes rather than the quantities of the solid phases.

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