Question

gas stoichiometry
for these problems, remember that the volumes are proportional to the stoichiometric coefficients!
question 18
1/3 pts 4-5 19 details
part 1 of 2
when fluorine gas combines with water vapor, the following reaction occurs:
$2f_2 + 2h_2o \
ightarrow o_2 + 4hf$
the reaction starts with 7 l of fluorine gas, how many liters of water vapor are needed to completely react the fluorine?
7l
part 2 of 2
how many liters of oxygen and hydrogen fluoride are produced?
oxygen gas:
hydrogen fluoride:
submit question
question 19
0/3 pts 5 19 details
part 1 of 2
nitrogen and oxygen gases react to form dinitrogen oxide gas ($n_2o$). what volume of $o_2$ is needed to produce 7.84 l of $n_2o$
balanced equation:

Explanation:

Step1: Determine the mole ratio for \(O_2\)

From the reaction \(2F_2 + 2H_2O
ightarrow O_2 + 4HF\), the ratio of \(F_2\) to \(O_2\) is \(2:1\). Given \(V_{F_2}=7\space L\), let \(V_{O_2}\) be the volume of \(O_2\). Using the volume - ratio (since volumes are proportional to moles for gases at same conditions), \(\frac{V_{F_2}}{V_{O_2}}=\frac{2}{1}\). So \(V_{O_2}=\frac{1}{2}\times V_{F_2}\). Substituting \(V_{F_2} = 7\space L\), we get \(V_{O_2}=\frac{7}{2}=3.5\space L\).

Step2: Determine the mole ratio for \(HF\)

The ratio of \(F_2\) to \(HF\) is \(2:4 = 1:2\). Let \(V_{HF}\) be the volume of \(HF\). Then \(\frac{V_{F_2}}{V_{HF}}=\frac{2}{4}=\frac{1}{2}\). So \(V_{HF}=2\times V_{F_2}\). Substituting \(V_{F_2}=7\space L\), we get \(V_{HF}=2\times7 = 14\space L\).

Answer:

Oxygen gas: \(3.5\space L\)
Hydrogen Fluoride: \(14\space L\)