Question

incorrect
your answer is wrong. in addition to checking your math, check that you used the right data and did not round any intermediate calculations.
fluorine gas and water vapor react to form hydrogen fluoride gas and oxygen. what volume of oxygen would be produced by this reaction if 1.2 cm³ of water were consumed?
also, be sure your answer has a unit symbol, and is rounded to the correct number of significant digits

Explanation:

Step1: Write the balanced chemical equation

The reaction between fluorine gas (\(F_{2}\)) and water vapor (\(H_{2}O\)) is \(2F_{2}+2H_{2}O = 4HF+O_{2}\).

Step2: Use the volume - ratio from the stoichiometry

From the balanced equation, the ratio of \(H_{2}O\) to \(O_{2}\) is \(2:1\) in terms of moles. At the same temperature and pressure (assuming ideal gas behavior, since we are dealing with gas volumes and the reaction involves gases), the ratio of volumes is the same as the mole - ratio (Avogadro's law: \(V = n\times V_{m}\), where \(V_{m}\) is the molar volume and is constant for a given \(T\) and \(P\)).
If \(V_{H_{2}O}=1.2\ cm^{3}\), and \(\frac{V_{H_{2}O}}{V_{O_{2}}}=\frac{2}{1}\) (from the stoichiometric coefficients of \(H_{2}O\) and \(O_{2}\) in the balanced equation).
Then \(V_{O_{2}}=\frac{V_{H_{2}O}}{2}\)

Step3: Calculate the volume of \(O_{2}\)

Substitute \(V_{H_{2}O}=1.2\ cm^{3}\) into the formula \(V_{O_{2}}=\frac{1.2\ cm^{3}}{2}\)

Answer:

\(0.60\ cm^{3}\)