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Q2) In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition of sodium azide (NaN₃) to its elements. A 43.398 g sample of sodium azide was decomposed, and the nitrogen gas generated was collected over water at 22°C. The total pressure was 798.8 mmHg. How many liters of dry N₂ were generated?

Q3) An atmospheric chemist studying the pollutant SO₂ places a mixture of SO₂ and O₂ in a1.14 L container at 825.7 K and 2.3 atm. When the reaction occurs, gaseous SO₃ forms, and the pressure falls to 1.26 atm. How many moles of SO₃ form?

Q4)

An environmental engineer analyzes a sample of air contaminated with sulfur dioxide. To a 466.03 mL sample at 727.1 torr and 46.9°C, she adds 20.58 mL of 0.01 M aqueous iodine, which reacts as follows:

Excess I₂ reacts with 13 mL of 0.014 M sodium thiosulfate:

What is the volume % of SO₂ in the air sample?

Q5) By what factor would a scuba diver's lungs expand if she ascended rapidly to the surface from a depth of 127.8 ft without inhaling or exhaling? If an expansion factor greater than 1.74 causes lung rupture, how far could she safely ascend from 127.8 ft without breathing? Assume constant temperature (d of seawater = 1.094 g/mL; d of Hg = 13.802 g/mL). Hint: The pressure at the surface is 1.00atm

Q6) Acrylic acid (CH₂ CHCOOH) is used to prepare polymers, adhesives, and paints. The first step in making acrylic acid involves the vapor-phase oxidation of propylene (CH₂ CHCH₃) to acrolein (CH₂ CHCHO). This step is carried out at 398.5°C and 4.8 atm in a large bundle of tubes around which a heat transfer agent circulates. The reactants spend an average of 1.5 s in the tubes, which have a void space of 98.5 ft³. How many mols of propylene must be added per hour in a mixture whose mole fractions are 0.07 propylene, 0.35 steam, and 0.58 air?

Q7) How many liters of gaseous hydrogen bromide at 21.2°C and 1.043 atm will a chemist need if she wishes to prepare 3.86 L of 2.367 M hydrobromic acid?

Q8) In the 19^th century, J. B. A. Dumas devised a method for finding the molar mass of a volatile liquid from the volume, temperature, pressure, and mass of its vapor. (next column). He placed a sample of such a liquid in a flask that was closed with a stopper fitted with a narrow tube, immersed the flask in a hot water bath to vaporize the liquid, and then cooled the flask. Find the molar mass of a volatile liquid from the following:

Mass of empty flask = 65.347 g

Mass of flask filled with water at 25°C = 327.4 g

Density of water at 25°C = 0.997 g/mL

Mass of flask plus condensed unknown liquid = 65.739 g

Barometric pressure = 104.5 kPa

Temperature of water bath = 99°C

SO2(g) + 2(aH20 HSO4 (aq) I(a)H(a unbalanced) 2aq) S.03(aq) > I(aS40 unbalanced atm Narrow tube gas Known V Known T>boiling point of liquid Heater

Answer 1

The volume velime Pterr KJOw the vale n trmula 65,01 V 0.6675 62 363 x 29s 798-8 V1223/-136 778-5