At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO3:

2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) ΔH = - 89.4 kJThe decomposition of KClO3 proceeds spontaneously when it is heated. Do you think that the reverse reaction, the formation of KClO3 from KCl and O2, is likely to be feasible under ordinary conditions? Explain.

Question

Sophie Davila

Chemistry

12 April, 07:03

At one time, a common means of forming small quantities of oxygen gas in the laboratory was to heat KClO3:

2 KClO3 (s) → 2 KCl (s) + 3 O2 (g) ΔH = - 89.4 kJThe decomposition of KClO3 proceeds spontaneously when it is heated. Do you think that the reverse reaction, the formation of KClO3 from KCl and O2, is likely to be feasible under ordinary conditions? Explain.

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Answers (1)

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Eugene Yoder · Answer 1

The reverse reaction is not feasible under ordinary condition

Explanation:

The forward reaction is highly exothermic and spontaneous under ordinary condition, hence the oxygen molecules cannot recombine with the KCl molecules to form KClO3 molecules under ordinary condition