4.3 Stoichiometry of gaseous substances, mixtures, and reactions  (Page 9/13)

Automobile air bags are inflated with nitrogen gas, which is formed by the decomposition of solid sodium azide (NaN ₃ ). The other product is sodium metal. Calculate the volume of nitrogen gas at 27 °C and 756 torr formed by the decomposition of 125 g of sodium azide.

Lime, CaO, is produced by heating calcium carbonate, CaCO ₃ ; carbon dioxide is the other product.

(a) Outline the steps necessary to answer the following question: What volume of carbon dioxide at 875° and 0.966 atm is produced by the decomposition of 1 ton (1.000 $\times$ 10 ³ kg) of calcium carbonate?

(b) Answer the question.

Before small batteries were available, carbide lamps were used for bicycle lights. Acetylene gas, C ₂ H ₂ , and solid calcium hydroxide were formed by the reaction of calcium carbide, CaC ₂ , with water. The ignition of the acetylene gas provided the light. Currently, the same lamps are used by some cavers, and calcium carbide is used to produce acetylene for carbide cannons.

(a) Outline the steps necessary to answer the following question: What volume of C ₂ H ₂ at 1.005 atm and 12.2 °C is formed by the reaction of 15.48 g of CaC ₂ with water?

(b) Answer the question.

Calculate the volume of oxygen required to burn 12.00 L of ethane gas, C ₂ H ₆ , to produce carbon dioxide and water, if the volumes of C ₂ H ₆ and O ₂ are measured under the same conditions of temperature and pressure.

What volume of O ₂ at STP is required to oxidize 8.0 L of NO at STP to NO ₂ ? What volume of NO ₂ is produced at STP?

Consider the following questions:

(a) What is the total volume of the CO ₂ ( g ) and H ₂ O( g ) at 600 °C and 0.888 atm produced by the combustion of 1.00 L of C ₂ H ₆ ( g ) measured at STP?

(b) What is the partial pressure of H ₂ O in the product gases?

Methanol, CH ₃ OH, is produced industrially by the following reaction:
$\text{CO}\left(g\right)+2{\text{H}}_2(g)\stackrel{\text{copper catalyst 300 °C, 300 atm}}{\to }{\text{CH}}_3\text{OH}\left(g\right)$

Assuming that the gases behave as ideal gases, find the ratio of the total volume of the reactants to the final volume.

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 BaO ₂ to BaO and O ₂ ?

A 2.50-L sample of a colorless gas at STP decomposed to give 2.50 L of N ₂ and 1.25 L of O ₂ at STP. What is the colorless gas?

Ethanol, C ₂ H ₅ OH, is produced industrially from ethylene, C ₂ H ₄ , by the following sequence of reactions:
$3{\text{C}}_2{\text{H}}_4+2{\text{H}}_2{\text{SO}}_4⟶{\text{C}}_2{\text{H}}_5{\text{HSO}}_4+{\left({\text{C}}_2{\text{H}}_5\right)}_2{\text{SO}}_4$
${\text{C}}_2{\text{H}}_5{\text{HSO}}_4+{\left({\text{C}}_2{\text{H}}_5\right)}_2{\text{SO}}_4+3{\text{H}}_2\text{O}⟶3{\text{C}}_2{\text{H}}_5\text{OH}+2{\text{H}}_2{\text{SO}}_4$

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%?

One molecule of hemoglobin will combine with four molecules of oxygen. If 1.0 g of hemoglobin combines with 1.53 mL of oxygen at body temperature (37 °C) and a pressure of 743 torr, what is the molar mass of hemoglobin?

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 fluoride in the original sample? (Note: Xenon fluorides contain only one xenon atom per molecule.)

One method of analyzing amino acids is the van Slyke method. The characteristic amino groups (−NH ₂ ) in protein material are allowed to react with nitrous acid, HNO ₂ , to form N ₂ gas. From the volume of the gas, the amount of amino acid can be determined. A 0.0604-g sample of a biological sample containing glycine, CH ₂ (NH ₂ )COOH, was analyzed by the van Slyke method and yielded 3.70 mL of N ₂ collected over water at a pressure of 735 torr and 29 °C. What was the percentage of glycine in the sample?
${\text{CH}}_2\left({\text{NH}}_2\right){\text{CO}}_2\text{H}+{\text{HNO}}_2⟶{\text{CH}}_2\left(\text{OH}\right){\text{CO}}_2\text{H}+{\text{H}}_2\text{O}+{\text{N}}_2$