9.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions

Calculate the density of Freon 12, CF₂Cl₂, at 30.0 °C and 0.954 atm.

A cylinder of O₂(g) used in breathing by patients with emphysema has a volume of 3.00 L at a pressure of 10.0 atm. If the temperature of the cylinder is 28.0 °C, what mass of oxygen is in the cylinder?

What is the molar mass of a gas if 0.281 g of the gas occupies a volume of 125 mL at a temperature 126 °C and a pressure of 777 torr?

The density of a certain gaseous fluoride of phosphorus is 3.93 g/L at STP. Calculate the molar mass of this fluoride and determine its molecular formula.

A 36.0–L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO₂, 805 g O₂, and 4,880 g N₂. At 25 degrees C, what is the pressure in the cylinder in atmospheres?

A sample of gas isolated from unrefined petroleum contains 90.0% CH₄, 8.9% C₂H₆, and 1.1% C₃H₈ at a total pressure of 307.2 kPa. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)

Most mixtures of hydrogen gas with oxygen gas are explosive. However, a mixture that contains less than 3.0 % O₂ is not. If enough O₂ is added to a cylinder of H₂ at 33.2 atm to bring the total pressure to 34.5 atm, is the mixture explosive?

A sample of carbon monoxide was collected over water at a total pressure of 756 torr and a temperature of 18 °C. What is the pressure of the carbon monoxide? (See the table for the vapor pressure of water.)

Joseph Priestley first prepared pure oxygen by heating mercuric oxide, HgO:
$2 \text{HgO} \left(s\right) \rightarrow 2 \text{Hg} \left(l\right) + \text{O}_{2} \left(g\right)$

(a) Outline the steps necessary to answer the following question: What volume of O₂ at 23 °C and 0.975 atm is produced by the decomposition of 5.36 g of HgO?

(b) Answer the question.

The chlorofluorocarbon CCl₂F₂ can be recycled into a different compound by reaction with hydrogen to produce CH₂F₂(g), a compound useful in chemical manufacturing:
$\text{CCl}_{2} \text{F}_{2} \left(g\right) + 4 \text{H}_{2} \left(g\right) \rightarrow \text{CH}_{2} \text{F}_{2} \left(g\right) + 2 \text{HCl} \left(g\right)$

(a) Outline the steps necessary to answer the following question: What volume of hydrogen at 225 atm and 35.5 °C would be required to react with 1 ton (1.000 $\times$ 10³ kg) of CCl₂F₂?

(b) Answer the question.

Lime, CaO, is produced by heating calcium carbonate, CaCO₃; carbon dioxide is the other product.

(a) Outline the steps necessary to answer the following question: What volume of carbon dioxide at 875 K and 0.966 atm is produced by the decomposition of 1 ton (1.000 $\times$ 10³ kg) of calcium carbonate?

(b) Answer the question.

Calculate the volume of oxygen required to burn 12.00 L of ethane gas, C₂H₆, to produce carbon dioxide and water, if the volumes of C₂H₆ and O₂ are measured under the same conditions of temperature and pressure.

Consider the following questions:

(a) What is the total volume of the CO₂(g) and H₂O(g) at 600 °C and 0.888 atm produced by the combustion of 1.00 L of C₂H₆(g) measured at STP?

(b) What is the partial pressure of H₂O in the product gases?

What volume of oxygen at 423.0 K and a pressure of 127.4 kPa is produced by the decomposition of 129.7 g of BaO₂ to BaO and O₂?

Ethanol, C₂H₅OH, is produced industrially from ethylene, C₂H₄, by the following sequence of reactions:
$3 \text{C}_{2} \text{H}_{4} + 2 \text{H}_{2} \text{SO}_{4} \rightarrow \text{C}_{2} \text{H}_{5} \text{HSO}_{4} + \left(\text{C}_{2} \text{H}_{5}\right)_{2} \text{SO}_{4}$
$\text{C}_{2} \text{H}_{5} \text{HSO}_{4} + \left(\text{C}_{2} \text{H}_{5}\right)_{2} \text{SO}_{4} + 3 \text{H}_{2} \text{O} \rightarrow 3 \text{C}_{2} \text{H}_{5} \text{OH} + 2 \text{H}_{2} \text{SO}_{4}$

What volume of ethylene at STP is required to produce 1.000 metric ton (1000 kg) of ethanol if the overall yield of ethanol is 90.1%?

A sample of a compound of xenon and fluorine was confined in a bulb with a pressure of 18 torr. Hydrogen was added to the bulb until the pressure was 72 torr. Passage of an electric spark through the mixture produced Xe and HF. After the HF was removed by reaction with solid KOH, the final pressure of xenon and unreacted hydrogen in the bulb was 36 torr. What is the empirical formula of the xenon…