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Why was the percentage recovery less than 100%? Give several reasons.
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- Why is the percent recovery of the essential oil less than 100%? State at least two reasons that are inherent to the experiment as performed and are thus unavoidable.16. The combustion of gasoline (octane) in a car engine can be represented by the following equation: 2C3H18(1) + 2502(g) a. What mass of oxygen is used up to burn a full tank of 36.00 kg of gasoline? Text --> 16CO2(g) +18H20(g) b. Why might a vehicle that is calibrated to run perfectly at sea level run poorly at higher elevations? Text Тext According to the Canadian Automobile Association, the average Canadian drives 20,000 km/yr. C. Assuming that distance, how many more kg of carbon dioxide are added to the atmosphere each year by a Toyota Tacoma (fuel economy of 12.8 L/100 km) than a Toyota Prius (4.52 L/100 km)? The density of gasoline is 0.719 kg/L.The following information was recorded by a student team working to prepare nickel sulfate. Plan: Prepare NiSO4 by reacting NiO with 6 M H2SO4 The expected product is NiSO4·6H2O. We will filter the crystals from the reaction solution to get the product. NiO + H2SO4 --> NiSO4 + H2O molar mass of NiO: 74.69 g/molmolar mass of NiSO4: 154.75 g/mol molar mass of NiSO4·6H2O: 262.85 g/mol mass of NiO used: 7.5 gvolume of 6M H2SO4 used: 50 mL heated the solution for 30 minutes, cool and filtered the crystals mass of product: 17.4 g Two students calculated percent yield using this data. One student got 66.2% and another got 112%. Based on this information, which of the following statements are true. One or more statements are correct. Group of answer choices The percent yield of 112% was calculated using the molar mass for the hydrated product. The percent yield of 66.2% was calculated using the molar mass for the anhydrous product. Both percent yields are incorrect because…
- 2b) What is the primary consideration?The great French chemist Antoine Lavoisier discovered the Law of Conservation of Mass in part by doing a famous experiment in 1775. In this experiment Lavoisier found that mercury(II) oxide, when heated, decomposed into liquid mercury and an invisible and previously unknown substance: oxygen gas. 1. Write a balanced chemical equation, including physical state symbols, for the D-0 decomposition of solid mercury(II) oxide (HgO) into liquid mercury and gaseous dioxygen. 2. Suppose 54.0 mL of dioxygen gas are produced by this reaction, at a temperature of 50.0 °C and pressure of exactly 1 atm. Calculate the mass of mercury(II) oxide that must have reacted. Round your answer to 3 significant digits. APR 24 MacBook AirThe 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 0.127-g sample of a compound was treated as above, producing 89.0 mL of N2 saturated with water vapor at 25 °C and 739.3 torr.What is the mass percent of nitrogen in the compound? . The vapor pressure of water at 25 °C is 23.8 torr.
- You work in a research organization that is looking for markers of various diseases that can be used as a diagnostic for the disease. It has been reported in the past that high levels of Cu are found in the sweat of people with cystic fibrosis. One of the research projects is focused on looking for high levels of Cu in samples that can be obtained non-invasively such as saliva, sweat, hair, nails, etc. The lab will analyze large samples for Cu. What instrument would you recommend purchasing to support this work, Atomic absorption spectrophotometer or an inductively coupled plasma atomic spectrophotometer? Explain the basis for your decision.NO(g) NO;(g) 90.25 210.7 86.57 33.2 240.0 51.30 N,O(g) N;O,(g) 82.05 219.7 104.2 83.72 321.28 139.46 (S)*O°N_ (3)*O°N 9.16 304.2 97.82 11 356 115 N,O;(s) -43.1 178 114 NOCI(g) HNO,(€) HNO,(g) 52.59 264 66,36 -174.1 155.6 -80.79 -135.1 266.2 -74.77 HNO, (aq) -206.6 146 -110.5 Hydrogen H(g) 218.0 114.6 203.3 H;(g) 130.6 H,O(€) -285.8 69.91 -237.2 H,O(g) -241.8 188.7 -228.6 H;O;() -187.8 109.6 -120.4 Cbromium Cr(s) 23.8 Cr,O;(s) Cr,Cl;(s) -1139.7 81.2 - 1058.1 -556.5 123.0 -486.1 (NH,) ¿Cr,O;(s) -1807 A -299.9 kJ/mol В 3,913.9 kJ/mol 299.9 kJ/mol D -3,913.9 kJ/molThe reaction for the Haber process, the industrial production of ammonia, is N2(8) + 3H2(8) – 2NH3(8) Assume that under certain laboratory conditions ammonia is produced at the rate of 6.29 mol L-1 s1. At what rate is hydrogen consumed? Round your answer to 2 decimal places.
- The density of moist air (ideal gas mixture) at 20°C temperature and 700 mmHg pressure was found to be 1.1 g/lt. Calculate the partial pressure of water vapor in this air. Additional data: MA(H2O)18, MA (Air)291) Listen -5 The Ksp value for calcium sulfate [CaSO4] is 2.40 X 10 and a professor made 1825 mL of a CaSO4(ag) solution but then one of his graduate student accidentally poured in a 0.125 M solution of calcium phosphate [Cag(PO4)2] solution. You may ignore the additional volume coming from the Ca3(PO4)2 solution to make the calculation simpler. Calculate the new sulfate (SO42) ion concentration at equilibrium with this common ion effect. 6.40 x 10-5 5.25 x 10-5 6.21 x 10-5 5.44 x 10-5 201591..docx LAB EXP. #3 -..docx Show All1. CH31 (excess) 2. Ag20, H2O, heat NH2