Consider this reaction at equilibrium.
\(2 \mathrm{KClO}_{3}(s) \rightleftharpoons 2 \mathrm{KCl}(s)+3 \mathrm{O}_{2}(g)\)
Predict the effect (shift right, shift left, or no effect) of these changes.
(a) adding \(\mathrm{KCl}\) to the reaction mixture
(b) adding \(\mathrm{KClO}_{3}\) to the reaction mixture
(c) adding \(\mathrm{O}_{2}\) to the reaction mixture
(d) removing \(\mathrm{O}_{2}\) from the reaction mixture
Equation Transcription:
Text Transcription:
2KClO_3(s) rightleftharpoons 2KCl(s)+3O_2(g)
KCl
KClO_3
O_2
Step 1
From this given equilibrium reaction
We have to predict the effect (shift right, shift left, or no effect) of these changes.
(a) adding KCl to the reaction mixture
(b) adding KClO3 to the reaction mixture
(c) adding O2 to the reaction mixture
(d) removing O2 from the reaction mixture
