Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) + (aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?

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Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes
spontaneously but slowly. The decomposition reaction will proceed at a
faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed
reaction are:
H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq)
OO
H₂O₂(aq) + Ol(aq) →
H₂O(l) + O₂(g) +1-(aq)
a. What is the net reaction?
b. If 10.00 mL of H₂O₂ undergoes this
reaction, what mass of oxygen is produced?
c. If the reaction has an 85.5% yield, what
mass of oxygen is actually produced?
Transcribed Image Text:Hydrogen peroxide, H₂O₂, has a density of 1.45 g/cm³ and decomposes spontaneously but slowly. The decomposition reaction will proceed at a faster rate if iodide ion, a catalyst, is added. The steps for the catalyzed reaction are: H₂O₂(aq) + (aq) → H₂O(l) + Ol-(aq) OO H₂O₂(aq) + Ol(aq) → H₂O(l) + O₂(g) +1-(aq) a. What is the net reaction? b. If 10.00 mL of H₂O₂ undergoes this reaction, what mass of oxygen is produced? c. If the reaction has an 85.5% yield, what mass of oxygen is actually produced?
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