answer the following questions?1-Paraffins are obtained by process from petroleum.| FiltrationSedimentation| fractional distillation| fermentation2-Corrosion in crude distillation unit column overhead system iscaused by.| All of the above| The sulphur compounds in crude oils| The presence of naphthenic acid in crude oils| The presence of HCL formed by dissociation of chloride salts3-Viscosity means the flow of the liquid is resisted by.| Alcoholother liquid| Water| Itself4-Pipeline operators to be equipped with.| Fire Fire truck| Safety shoes| refrigerated work suitsvapour pressure analyser5-Aromatic compounds are produced from.| coal tar| oil gas| heavy gasnatural gas6-If the crude is paraffinic then its characterization factor will be.目11目5目8| Above 127_Which of the following statements is true if a fuel has a highaniline point.| Fuel has high diesel index| Fuel has high aromatics| Fuel ha low paraffin| Fuel has low diesel index8-Which of the following hydrocarbons with the following APIgravity has the highest Sulphur content?目10| 20| 30目409-What Does Aviation Fuel Contain?| Light Naphtha| Medium Naphtha| KeroseneI Diese10-Metallic compounds can be found in all crude oil in ?low low concentration| trace levelsmeddle concentrationhigh concentration

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answer the following questions? 1-Paraffins are obtained by process from petroleum. | Filtration | Sedimentation | fractional distillation | fermentation 2-Corrosion in crude distillation unit column overhead system is caused by. | All of the above The sulphur compounds in crude oils | The presence of naphthenic acid in crude oils | The presence of HCL formed by dissociation of chloride salts 3-Viscosity means the flow of the liquid is resisted by. | Alcohol | other liquid | Water | Itself

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter5: Distillation

Section: Chapter Questions

Problem 4Q

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pure liqu PB liquid x solution B Esure solid x liquid x (saturate»
Table 1. Experimentally Determined Changes in Freezing Point for Aqueous Solutions Substance Freezing Point Tr (°C) AT = T°r-T Trial 1 -0.1°C Pure Water Pure Water Trial 2 T=-04°C Average Tr= -1-5 °C NaCI/Water Solution Ethylene Glycol/Water Solution Tr= 0.2 °C -3:2°C - 3 T2 Tr- A°C -49°C - 6 TS Methanol/Water Solution (Amoles (6.02X10 Table 2. Three Ratios for Specifying the Composition of Aqueous Solutions gsolute/gsolvent mole,olutegsolvent moleparticles/gsolvent Substance 5.029/5M •085q /sg 59 5-121 102 NaCI/Water Solution 5.05X10" L 5g . 0147 na 0.85X16) 5g .0434 /59 523/5m 5M Ethylene Glycol/Water Solution Methanol/Water Solution 1. Might any of the ratios you calculated for Table 2 above be useful for predicting how the freezing point of a solution would differ from that of the pure liquid? Explain.
20 Enter your answer in the provided box. The solubility of CO, in water at 25°C and 1 atm is 0.034 mol/L. What is its solubility at a partial pressure in air of 0.00031 atm? Assume that CO, obeys Henry's law. X 01:25:27 mol / L Mc Graw < Prev Next 20 of 20 .. 114H
Extra information: freezing point depression constant for the solvent (20.0 degrees Celcius kg/mol for cyclohexane)
A solution containing 10.0 % sodium sulfate by weight is cooled to 32° F, where the solid phase is the decahydrate and the solubility of the sodium sulfate is 0.634 mol per 100 mols of water. What is the resulting slurry density in pounds solids per 100 pounds of total mix?
A batch of 500 ?? of ??? dissolves in water to form a saturated solution at 350 ? (77 °?) where the solubility is 30% by weight of ??? in water. The solution cools at 293 ? (20 °?) at which the solubility is 25.4% by weight. Determine the number of crystals obtained if 3.5% of the original water evaporates on cooling. Also, determine the capacity of the container in which this solution is cooled if it is 1.20 times the volume of the solution. The density of the solution is ???? ??/??
The solubility of KNO3 at 25°C is 80 g KNO3 / 100g H20. [ Select ] solution a) A solution of 160g KNO3 in 200g of water is a [ Select ] unsaturated saturated supersaturated Stittt J solution b) A solution of 45g KNO3 in 50g of water is a [ Select ] v solution c) A solution of 10g KNO3 in 25g of water is a
Which of the following statements about fractional distillation are true.? Select all that are True. A)The lower the HETP (height equivalent to a theoretical plate) of the fractionating(packed) column the more efficient it is at separation of components. B)The distillation process involves several concurrent vaporization-condensation cycles. C)Continual change in boiling temperature is observed as the distillation progresses. D)Can ideally separate mixtures with comparable volatilities small BP differences. E)For good separation by distillation the volume of liquid condensing back to the pot should be lower than the volume of liquid distilling off.
- 2022.pdf - Adobe Acrobat Pro DC (32-bit) ndow Help oter 14 - Soluti. x 2 / 3 100% 9) An aqueous solution has a normal boiling point of 103.0°C. What is the freezing point of this solution? For water Kb = 0.51°C/m and Kf=1.86°C/m. 9) A) -0.82°C B) -3.0°С С) -3.6°C D) -11°C 10) A solution of an 22.4 g of an unknown protein dissolved in enough water to make 0.150 L of solution has an osmotic pressure of 658 torr at 25°C. Based on these data, what is the molar mass of the protein? 10) search hp
ite arses/2015/assignments/7920 Week 5: Freezing Point Depression of Non-Electrolytes Methanol in Water 10.00 1.00 Data and Calculations: Pure Water 10.00 Volume of Water (ml) Mass of Methanol (g) Freezing Point ('C) Freezing point depression AT Calculate the molality m (K, = 1.86 °C/m for water) Calculate number of moles Tsotution = -4.5 Tsolzent = 1 AT, = Tsotvent – Tsotution = AT = Kf.m→ m = AT;/Kf = m = moles methanol/ Kg solvent → moles methanol = m x Kg solvent = moles methanol = mass methanol /molar mass methanol → molar mass methanol = mass methanol / moles methanol → molar mass methanol = 1.00 g/ moles methanol Calculate the molar mass of methanol e error (actual molar mass of methanol = % error =[ ]actual – experimental| / actual ] x 100% 32.04 g/mol) Question: 1. What is the freezing point of a solution prepared by dissolving 20 g of ethanol (Molar mass = 46 g/mol) in 120 ml. of water? The freezing point depression constant K, for water is 1.86 °C/m. Assume density of water…
ngage.com/static/nb/ui/evo/index.html?elSBN=9781305... * MINDTAP Q Search this course il. Use the References to access important values if needed for this question. The common laboratory solvent benzene is often used to purify substances dissolved in it. The vapor pressure of benzene, C,H6, is 73.03 mm Hg at 25 °C. The molecular weight of benzene, C6H6, is 78.12 g/mol. In a laboratory experiment, students synthesized a new compound and found that when 14.29 grams of the compound were dissolved in 152.3 grams of benzene, the vapor pressure of the solution was 71.22 mm Hg. The compound was also found to be nonvolatile and a nonelectrolyte. What is the molecular weight of this compound? MW g/mol Submit Answer
-Lab. II. Freezing point of a pure solid. Data Table. mass of pure naphthaleneo il1.3119 * 2. Freezing (melting ) point of naphthalene10.4 III. Molecular weight by freezing point depression. dEISI Data Table 1. mass of unknown * 2. Freezing (melting ) point of solution 72.3°0 Calculation (Carry out to proper number of significant digits.) 1. AT (difference in freezing points of pure naphthalene and solution) AT= oN awominU 2. molecular weight of unknown solute AT=Kfgmi KP Naph =7.0°Gt molal 7.0°%/molal