The equilibrium constant for the reaction Fe3 O4(s)+CO(g) 3 FeO(s)+CO2(g) at 600 C is 1.00. If a mixture initially consisting of 1 mole of Fe3 O4, 2 moles of CO, 0.5 mole of FeO and 0.3 mole of CO2 is heated to 600 C at constant total pressure of 5 atmosphere, how many moles of each substance would be present at equilibrium ?

ABC26PH0640 · Chemical Equilibrium

Subject: Physical Chemistry · Chapter: Chemical Equilibrium · Topic: Chemical Equilibrium – General · Exam: JAM 2001-2022 · Marks: 2 · Difficulty: Medium

The equilibrium constant for the reaction

\[ \mathrm{Fe}_{3} \mathrm{O}_{4}(\mathrm{s})+\mathrm{CO}(\mathrm{g}) \rightleftharpoons 3 \mathrm{FeO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g}) \]

at $600^{\circ} \mathrm{C}$ is 1.00. If a mixture initially consisting of 1 mole of $\mathrm{Fe}_{3} \mathrm{O}_{4}, 2$ moles of $\mathrm{CO}, 0.5$ mole of FeO and 0.3 mole of $\mathrm{CO}_{2}$ is heated to $600^{\circ} \mathrm{C}$ at constant total pressure of 5 atmosphere, how many moles of each substance would be present at equilibrium ?

Answer

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Explanation

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