The CO2 produced from the combustion of Molecule 1 is collected over water at a total pressure of 741 mm Hg, 30.0 oC and a volume of 178 mL. Calculate the partial pressure of CO2 and the grams of Molecule 1 consumed.
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- 5-118 Isooctane, which has a chemical formula C8H18 is the component of gasoline from which the term octane rating derives. (a) Write the balanced chemical equation for the combustion of isooctane. (b) The density of isooctane is 0.792 g/mL. How many kg of C02 are produced each year by the annual U.S. gasoline consumption of L? (c) What is the volume in liters of this CO2 at STP? (d) The chemical formula for isooctane can be represented by (CH3)3CCH2CH(CH3)2. Draw a Lewis structure of isooctane. (e) Another molecule with the same molecular formula is octane, which can be represented by: When comparing isooctane and octane, one structure is observed to have a boiling point of 99°C, while another is known to have a boiling point Of 125°C. Which substance, isooctane or octane, is expected to have the higher boiling point? (f) Determine whether isooctane or octane is expected to have the greater vapor pressure.To apply a green chemistry approach, a chemical engineer uses waste CO₂ from a manufacturing process, instead of chlorofluorocarbons, as a “blowing agent” in the pro-duction of polystyrene containers. Find the density (in g/L) of CO₂ and the number ofmolecules per liter (a)at STP (0°C and 1 atm) and (b)at room conditions (20°.C and1.00 atm).The nitrogen content of organic compounds can be determined by the Dumas method.The compound in question is first passed over hot CuO(s): Compound ----> N2(g) + CO2(g) + H2O(g) The gaseous products are then passed through a concentrated aqueous KOH solution to remove the CO2.The remaining gas contains N2 and water vapor.A 0.185-g sample of a compound was treated as above, producing 82.2 mL of N2 saturated with water vapor at 25 °C and 775.0 torr.What is the mass percent of nitrogen in the compound? (The vapor pressure of water at 25 °C is 23.8 torr.)
- The complete combustion of 0.500 g of hydrocarbon, containing only C and H, produced 0.771 L of CO2 at STP and 0.755 g of water. In another experiment, 0.218 g of sample occupied 185 ml at 23 °C and 374 mm Hg. What is the molecular formula of the compound?Determine the mole fraction and partial pressure for each gas in the mixtures below.a) 1.62 g CO2 and 13.5 g XeF2 at STP.b) 679 mg He and 1.21 g NO2 in an 875-mL vessel at 26.3°C.Pressure (A) Explain the term pressure and state its S.I. unit. (B) Explain Henry’s law. (C)A bottle of H2 has just been received by the technicians in DkIT for use in the instrumentation lab. It is a 47 litre cylinder at a pressure of 50 atmospheres. The normal working pressures is 2 bar. (i) To what volume of gas will that equate at the working pressure? (ii) For how many hours will the gas last if it used at the rate of 0.5dm3 per hour? D)You see your best friend at the bar and you walk up behind her. You accidentally startle her and she takes a step backwards. Unfortunately, she is wearing high heels and her heels come down on your foot. She weighs only 55kg but the size of her heel is 6mm by 6mm.Determine the pressure that she applies on your foot. (E) If a diver dives to a depth of 35 m what will be: (i) the pressure in Pascals due the water column? (3 marks) (ii) the pressure of the air in…
- Aqueous sulfurous acid (H2SO3) was made by dissolving 0.200 L of sulfur dioxide gas at19°C and 745 mmHg in water to yield 500.0 mL of solution. The acid solution required 10.5 mL of sodium hydroxide solution to reach the titration end point. What was the molarity of the sodium hydroxide solution?Nitrogen content of an organic compound can be determined by the Dumas Method. The compound is passed over hot copper (II) oxide and reacts as follows: Compound N 2 + CO 2 + H 20The product gases are passed through a solution of potassium hydroxide to remove CO2. The remaining gas is N2 saturated with H20 vapour. In a given experiment 0.225g of the unknown compound produces 27.8mL of N2 saturated with H2O vapor at 25oC and 730Torr. What mass is the % of nitrogen in the compound? (NB: vapour pressure of H2O at this temperature is 23.8Torr.)Butane gas is stored in a cylinder at a pressure of 100 psig and at a temperature of 250C. Some of the butane gas was used and after some time, the pressure had gone down to 50 psig. If the temperature is 250C, what fraction of butane had been used?
- 1. The compressibility factor Z = PV/nRT for O2 at -27.1°C and 537.1 atm is 1.50; at 147.4°C and 95.5 atm, it is 1.02. A certain mass of oxygen occupied a volume of 3.28 L at 147.4°C and 95.5 atm. Calculate the volume occupied by the same quantity of oxygen at -27.1°C and 537.1 atm. 2. The composition of a mixture of gases in percentage by volume is 20.5% nitrogen, 15.7% carbon monoxide, 37.8% water, and the rest sulfur dioxide. Calculate the density of the gaseous mixture at 39.8°C and 1.46 atm in grams/liter. Report your answer to the hundredths position.Air at 25 degree celsium and 1 atm has 78% by volume N2, 21% by volume O2, and 0.05% by volume methyl ethyl ketone (MEK, CH3CH2COCH3) a) What is the concentration of each component in ppm b)What is the concentration of each in micrograms/cubic meterConsider the following chemical reactions: KClO3 (s) ----------> KCl(s) + O2(g) NaNO3(s) ---------> NaNO2(s) + O2(g) 5.0000 g mixture of potassium chlorate and sodium nitrate is decomposed and the mass of residuals is 3.8600 g. The oxygen gas is collected in 359. mL. container at 25 oC by water displacement technique. Calculate the total pressure in mmHg. the vapor pressure of H2O at 25oC is 18.3 mmHg. K = 39.10 g/mole, Cl = 35.45 g/mole, Na = 22.99 g/mole, N = 14.00 g/mole and O = 16.00 g/mole