a sample of h2 gas is collected over water at 23 degrese celsius, if the observed pressure is 750.0 torr, calculate the partial
1 answer:
Answer:
728.9 torr
Explanation:
Collecting a gas over water results in gathering a mixture of gases. First of all, the target gas is collected, but the gathered sample also contains saturated water vapor.
The saturated water vapor always produces the same pressure which depends on temperature. At a given temperature of 23 degrees Celsius, the saturated vapor pressure is equal to 21.1 torr.
The total pressure is equal to the sum of partial pressures of water and hydrogen:
Solving for the partial pressure of hydrogen:
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Answer:
5.52 g
Explanation:
- 4NH₃ + 5O₂ → 4NO + 6H₂O
First we <u>convert the given masses of both reactants into moles</u>, using their <em>respective molar masses</em>:
- 6.30 g NH₃ ÷ 17 g/mol = 0.370 mol NH₃
- 1.80 g O₂ ÷ 32 g/mol = 0.056 mol O₂
Now we <u>calculate with how many NH₃ moles would 0.056 O₂ moles react</u>, using the<em> stoichiometric coefficients</em>:
- 0.056 mol O₂ *
= 0.045 mol NH₃
As there more NH₃ moles than required, NH₃ is the excess reactant.
Then we calculate how many NH₃ moles remained without reacting:
- 0.370 mol NH₃ - 0.045 mol NH₃ = 0.325 mol NH₃
Finally we convert NH₃ moles into grams:
- 0.325 mol NH₃ * 17 g/mol = 5.52 g