The value K for H2(g) + CO2(g) <-> H2O(g) + CO(g) is 1.80 at 1000 C. If 1.0 mole of each H2 and CO2 are placed in 1 litre flask, the final equilibrium concentration of CO at 1000 C will be:
Correct answer: D. 0.573 M
- A. 0.295 M
- B. 0.385 M
- C. 0.531 M
- D. 0.573 M
Explanation
The given reaction is :- H2(g)+CO2(g)⇌H2O(g)+CO(g) Initial moles : 1 1 0 0 At eqm : 1−x 1−x x x Now, KC=[H2O][CO]/[H2][CO2] 1.8=x.x/(1-x)(1-x) ⇒x2=1.8(1−x)2 Taking square root on both sides ⇒x=1.34(1−x)⇒2.34x=1.34 ⇒x=0.573 So, concentration of CO at eqb=0.573M
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About Chemical Equilibrium
Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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