How many moles of oxygen gas can 0.88 mole of hydrogen peroxide \( \left(\mathrm{H}_{2} \mathrm{O}_{2}\right) \) produce, if decomposition is complete? \( 2 \mathrm{H}_{2} \mathrm{O}_{2} \rightarrow 2 \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2} \) \( \begin{array}{l}1.8 \text { moles } \\ 0.44 \text { mole } \\ 0.50 \text { mole } \\ 2.0 \text { moles } \\ 0.88 \text { mole } \\ \text { Submit Request Answer }\end{array} \)

In the decomposition of hydrogen peroxide \( (H_2O_2) \), the balanced equation indicates that 2 moles of \( H_2O_2 \) produce 1 mole of \( O_2 \). So, if you have 0.88 moles of \( H_2O_2 \), you can determine the moles of oxygen gas produced with a simple ratio: \( 0.88 \, \text{moles} \, H_2O_2 \times \left(\frac{1 \, \text{mole} \, O_2}{2 \, \text{moles} \, H_2O_2}\right) = 0.44 \, \text{moles} \, O_2 \). While we're talking about decomposition, did you know that hydrogen peroxide has been used in various historical contexts? It served as a key disinfectant in World War I and was later adapted in rocket propellants due to its ability to produce oxygen upon breakdown. Its versatility has made it a household staple as well as a part of industrial processes!