4.3 Stoichiometry of gaseous substances, mixtures, and reactions  (Page 8/13)

A 36.0–L cylinder of a gas used for calibration of blood gas analyzers in medical laboratories contains 350 g CO ₂ , 805 g O ₂ , and 4,880 g N ₂ . At 25 degrees C, what is the pressure in the cylinder in atmospheres?

A cylinder of a gas mixture used for calibration of blood gas analyzers in medical laboratories contains 5.0% CO ₂ , 12.0% O ₂ , and the remainder N ₂ at a total pressure of 146 atm. 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.)

A sample of gas isolated from unrefined petroleum contains 90.0% CH ₄ , 8.9% C ₂ H ₆ , and 1.1% C ₃ H ₈ 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.)

A mixture of 0.200 g of H ₂ , 1.00 g of N ₂ , and 0.820 g of Ar is stored in a closed container at STP. Find the volume of the container, assuming that the gases exhibit ideal behavior.

Most mixtures of hydrogen gas with oxygen gas are explosive. However, a mixture that contains less than 3.0 % O ₂ is not. If enough O ₂ is added to a cylinder of H ₂ at 33.2 atm to bring the total pressure to 34.5 atm, is the mixture explosive?

A commercial mercury vapor analyzer can detect, in air, concentrations of gaseous Hg atoms (which are poisonous) as low as 2 $\times$ 10 ⁻⁶ mg/L of air. At this concentration, what is the partial pressure of gaseous mercury if the atmospheric pressure is 733 torr at 26 °C?

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 [link] for the vapor pressure of water.)

In an experiment in a general chemistry laboratory, a student collected a sample of a gas over water. The volume of the gas was 265 mL at a pressure of 753 torr and a temperature of 27 °C. The mass of the gas was 0.472 g. What was the molar mass of the gas?

Joseph Priestley first prepared pure oxygen by heating mercuric oxide, HgO:
$2\text{HgO}\left(s\right)⟶2\text{Hg}\left(l\right)+{\text{O}}_2(g)$

(a) Outline the steps necessary to answer the following question: What volume of O ₂ at 23 °C and 0.975 atm is produced by the decomposition of 5.36 g of HgO?

(b) Answer the question.

Cavendish prepared hydrogen in 1766 by the novel method of passing steam through a red-hot gun barrel:
$4{\text{H}}_2\text{O}\left(g\right)+3\text{Fe}\left(s\right)⟶{\text{Fe}}_3{\text{O}}_4(s)+4{\text{H}}_2(g)$

(a) Outline the steps necessary to answer the following question: What volume of H ₂ at a pressure of 745 torr and a temperature of 20 °C can be prepared from the reaction of 15.O g of H ₂ O?

(b) Answer the question.

The chlorofluorocarbon CCl ₂ F ₂ can be recycled into a different compound by reaction with hydrogen to produce CH ₂ F ₂ ( g ), a compound useful in chemical manufacturing:
${\text{CCl}}_2{\text{F}}_2(g)+4{\text{H}}_2(g)⟶{\text{CH}}_2{\text{F}}_2(g)+2\text{HCl}\left(g\right)$

(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 $\times$ 10 ³ kg) of CCl ₂ F ₂ ?

(b) Answer the question.