A sample of hydrogen peroxide (H2O2\text{H}_2\text{O}_2H2O2) solution was decomposed in the presence of a manganese(IV) oxide catalyst:
2H2O2(aq)→2H2O(l)+O2(g) 2\text{H}_2\text{O}_2(\text{aq}) \rightarrow 2\text{H}_2\text{O}(\text{l}) + \text{O}_2(\text{g}) 2H2O2(aq)→2H2O(l)+O2(g)The reaction produced 145 cm3 of oxygen gas, measured at 21.0 ∘C21.0\text{ }^\circ\text{C}21.0 ∘C and 98.5 kPa.
What is the amount, in moles, of hydrogen peroxide that decomposed?
The gas constant, R=8.31 J K−1 mol−1R = 8.31\text{ J K}^{-1}\text{ mol}^{-1}R=8.31 J K−1 mol−1
2.92×10−32.92 \times 10^{-3}2.92×10−3
5.85×10−35.85 \times 10^{-3}5.85×10−3
1.17×10−21.17 \times 10^{-2}1.17×10−2
1.17×10−51.17 \times 10^{-5}1.17×10−5