At 1000°C, the equilibrium constant for the reaction of the system 2H2(g) + O2(g) ⇌ 2H2O(g) is very large. This implies that:
Correct answer: D. H2O(g) has very little tendency to decompose into H2(g) and O2(g) at I 000°C
- A. H2O(g) is unstable at 1000°C
- B. H2(g) is unstable at 1000°C
- C. H2 and O2 have very little tendency to combine at 1000°C
- D. H2O(g) has very little tendency to decompose into H2(g) and O2(g) at I 000°C
Explanation
High Kc values show product stability. A large equilibrium constant (K) implies that the reaction strongly favors the products. In this case, it means that H2O(g) has a very little tendency to decompose into H2(g) and O2(g) at 1000°C because the reaction overwhelmingly goes in the direction of forming H2O(g) (the products).
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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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