Help?
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 19th 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
Help? Q2) In a collision of sufficient force, automobile air bags respond by electrically trigger...
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? 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...
In a collision of sufficient force, automobile air bags respond by electrically triggering the explosive decomposition of sodium azide (NaN3) to its elements. A 58.6−g sample of sodium azide was decomposed, and the nitrogen gas generated was collected over water at 26°C. The total pressure was 733.2 mmHg. How many liters of dry N2 were generated?
The sodium azide required for automobile air bags is made by the reaction of sodium metal with dinitrogen monoxide in liquid ammonia: You have 62.8 g of sodium, a 35.5-L flask containing N2O gas with a pressure of 2.48 atm at 23 °C, and excess ammonia. What is the theoretical yield (in grams) of NaN3? 3 N2O (g) + 4 Na (s) + NH3 (l) ---> NaN3 (s) + 3 NaOH (s) + 2 N2 (g) Mass = g
Could someone assist me with this question? In the 19th 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...
1. Air bags are activated when a severe impact causes a steel ball to compress a spring and electrically ignite a detonator cap. This causes sodium azide (NaN3) to decompose explosively according to the following reaction: 2Na (s) 3N2 (g) 2NAN3 (s) 72.01 IL1,01(3) What mass of NaN3 (s) must be reacted to inflate an air bag to 70.0 L at 1 atm and 20°C? (8 pts.) 1273,15 293.15 21100,8 0V mol HOTS 3,31 X10 2. Exactly 50.0 mL liquid...
Part 1. The air in a bicycle tire is bubbled through water and collected at 25∘C. If the total volume of gas collected is 5.60 L at a temperature of 25∘C and a pressure of 760 torr, how many moles of gas were in the bicycle tire? - Part 2. A 295-mL flask contains pure helium at a pressure of 755 torr . A second flask with a volume of 480 mL contains pure argon at a pressure of 714...
i need part 2 and part 3 to be solved thanks please please urgent Instructor Name: Student Name: DATA (EXP #13): Part 1: The Action of Atmospheric Pressure Observations upon immersing the can in ice-water bath: Part 2: Determination of the Molar Mass of Gases Barometric pressure (mmHg): 734.2 mm Room temperature (0 23, 6"c CO2 Natural Gas Mass of flask/stopper filled with air (g) 126 069 125.959 la 0146-16 146.9 Volume of water used to fill flask (mL) 267-nL...
please show steps. thanks ! Experiment 19 Gas Stoichiometry and the Gas Laws The relationship between the physical properties of a gas, and the moles, is given by the “Ideal Gas Law:" PV=nRT where n-number of moles R=the ideal gas constant: 0.0821 atm L mole 'Kor 62.4 L torr molek In this experiment, the theoretical yield of gas, will be compared to the experimental yield. The reaction of aluminum with hydrochloric acid produces hydrogen according to the balanced equation below....
_ and _ bond(s) in the H2C-CH2 molecule. 25) There are A) 3 and 2 B) 3 and 4 C) 4 and 3 D) 2 and 3 E) 5 and 1 is tetrahedral 26) The electron-domain geometry of A) CBr4 B) PH3 C) CCl2Br2 D) XeF4 E) all of the above except XeF4 27) GeF3H is formed from GeH4 and GeF4 in the combination reaction: GeH4 + 3GeF4 + 4GeF3H If the reaction yield is 92.6%, how many moles of...
With the data given, help on the calculations please - Tes Name Determination of the Gas Constant, R, and the Purity of KCIO, Data Unknown number or letter Mass of test tube and iron (IIT) oxide 44.5928 Mass of test tube, iron (III) oxide and sample 44.979 8 Mass of test tube and contents after heating 44.8488 Volume of water displaced Barometric pressure 976 mbar Temperature of water temperature of O, 23 Vapor pressure of water at this temperature 21.068_mm...