Concept explainers
(a)
Interpretation:
The production rate of solid acetaminophen
Concept introduction:
In a system, a conserved quantity (total mass, mass of a particular species, energy or momentum) is balanced and can be written as:
Here, ‘input’ is the stream which enters the system. ‘generation’ is the term used for the quantity that is produced within the system. ‘output’ is the stream which leaves the system. ‘consumption’ is the term used for the quantity that is consumed within the system. ‘accumulation’ is used for the quantity which is builds up within the system.
From volumetric flowrate, mass flowrate is calculated if the density of the substance is given as:
Here,
(b)
Interpretation:
The reason on which the recovery of the stream (2) containing highly dilute acetaminophen can be processed is to be stated.
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Chapter 3 Solutions
EBK ELEMENTARY PRINCIPLES OF CHEMICAL P
- ou place hot metal into a beaker of cold water. ol type='a'> Eventually what is true about the temperature of the metal compared to that of the water? Explain why this is true. i>Label this process as endothermic or exothermic if we consider the system to be the metal. Explain. the water. Explain.arrow_forwardA solution is prepared by dissolving 10 g (NH:):SO4 in enough water to make 100.0 mL stock solution. A 11.00-mL sample of this stock solution is then placed in a 50.00-mL volumetric flask and diluted to the mark with water. What is the molarity of the new solution? (MW of (NH.)»SO« = 132.14 g/mol) %3Darrow_forwardYou have a flask weighing 121.214 g. To this flask, you added 25.00 mL KCl(aq) solution. You weigh the flask, it is now 150.234 g. You then take the flask to a heating source and evaporate all solvents. When the flask cool down to room temperature, you weigh the flask again, it is 124.231 g. What is the molality of the KCI (aq) solution? The amus for K is 39 and Cl is 35.5, respectivelyarrow_forward
- Hydrogen peroxide solutions can easily be decomposed by dust, trace amounts of metals or light. It istherefore necessary to periodically determine the purity of the peroxide solutions.This can be done via a redox titration as follows: The density of a particular surgical grade hydrogen peroxide solution is 1.11g.cm-3. Exactly 10 mL of this solution was pipetted and quantitatively transferred, along with a sufficientamount of a dilute sulphuric acid solution, into a 250.00 mL volumetric flask and made up to the mark. A 25.00 mL portion of this diluted solution is pipetted into a conical flask, and titrated with a0.372 M KMnO4 solution. The endpoint of the titration is determined when the colourless solution in the conical flask turns apersistent bright pink due to the presence of excess permanganate ions. The average titration value is 26.20 mL of the KMnO4 solution 1.Determine the percentage of the hydrogen peroxide in the solution sample.2. Naturally occurring manganese…arrow_forwardA chemistry student adds a quantity of an unknown solid compound X to 2.00 L of distilled water at 30.° C. After 10 minutes of stirring, only a little X has dissolved. The student then drains off the solution and evaporates the water under vacuum. A precipitate is left behind. The student washes, dries and weighs the precipitate. It weighs 0.052 kg. Using only the information above, can you calculate the solubility of X in water at 30.° C ? If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits. O yes O no 0 0x10 ロ・ロ X μ 00 3 4arrow_forwardA chemistry student adds a quantity of an unknown solid compound X to 450. mL of distilled water at 25.° C. After 10 minutes of stirring, only a little X has dissolved. The student then drains off the solution and evaporates the water under vacuum. A precipitate is left behind. The student washes, dries and weighs the precipitate. It weighs 94.5 g. O yes Using only the information above, can you calculate Ox10 the solubility of X in water at 25.° C? O no If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits.arrow_forward
- A chemistry student adds a quantity of an unknown solid compound X to 550. mL of distilled water at 30.° C. After 10 minutes of stirring, all of the Xhas dissolved. The student then drains off the solution and evaporates the water under vacuum. A precipitate is left behind. The student washes, dries and weighs the precipitate. It weighs 19.3 g. O yes Using only the information above, can you calculate the solubility of X in water at 30.° C? O no If you said yes, calculate it. Be sure your answer has a unit symbol and the right number of significant digits.arrow_forward✓- a Gasoline vaporizes in the carburetor of an automobile engine 2Hg (1) + O₂ (g) --> - 2HgO (s) seperating solute particles throughout a solvent SO₂(g) + CaO(s) -----> CaSO3(s) freezing water to form ice BaF2 (s)--> Ba2+ (aq) + 2F (aq) PCL3(g) + Cl₂(g) ----> PCL5 (g) melting ice to form water Raindrops form in a cloud | C₂H4(g) + H₂(g) ---> - C₂H6 (g) Ni(s) + 2 HCl(aq) -----> H₂(g) + NiCl₂(aq) Sugar dissolves in coffee CO₂(g) + H₂O(1) ----> H₂CO3(aq) 2NO₂ (g) - dissolution of solid KCl in water mixing of two gases into one container boiling water to form steam Frost forms on the windshield of your car --> N₂O4 (g) CaO(s) + 2 HCl(g) ---> CaCl₂(s) + H₂O(l) Moisture condenses on the outside of a cold glass ir is pumped into a tire Sub question a. As0arrow_forwardA sulfuric acid spill occurred on the highway after a truck containing barrels of sulfuric acid swerved out of control from a truck tire blowout. Luckily no one got hurt in the event but there is a concern that the sulfuric acid spill may affect local ground water supply. A sample of the ground water in that area was recovered to assess the extent of contamination of the ground water supply. In order to determine the concentration of sulfuric acid in the sample, 25.00 mL of the ground water sample was titrated with 0.133 M NaOH and you get the following data: Sodium hydroxide (initial buret reading) 0.66 mL Sodium hydroxide (final buret reading) 17.42 mL Calculate the molarity of sulfuric acid in the ground water sample. Enter numerical answer. Report in 3 sig figs. Show workarrow_forward
- When 20 grams of potassium chlorate, KCIO3, is dissolved in 100 grams of water at 80 °C, the solution can be correctly described as: 100 90 80 NANO, 70 Pb(NO)2 KNOS 60 CaC 50 O 40 NaCl KCI 30 20 KCIO, 10 Ce,(SO 10 20 30 40 50 60 70 80 90 100 Temperature ("C) supersaturated saturated unsaturated Solubility (g of salt in 100 g H,O) CONY 00 0 K,Cr,O,arrow_forwardIn a laboratory experiment, a fermenting aqueous solution of glucose and yeast produces carbon dioxide gas and ethanol. The solution was heated by burning natural gas in a Bunsen burner to distill the ethanol that formed in the flask. During the distillation, the ethanol evaporated and then condensed in the receiving flask. The flame of the burner was kept too close to the bottom of the flask and some of the glucose decomposed into a black carbon deposit on the inside of the flask. During this experiment the following changes occurred. Which of these changes involved a physical change and not a chemical change? Check all that apply. • View Available Hint(s) formation of a carbon deposit inside the flask O burning of natural gas formation of carbon dioxide gas from glucose condensation of ethanol formation of ethanol from glucose by yeast evaporation of ethanolarrow_forwardIn a laboratory experiment, a fermenting aqueous solution of glucose and yeast produces carbon dioxide gas and ethanol. The solution was heated by burning natural gas in a Bunsen burner to distill the ethanol that formed in the flask. During the distillation, the ethanol evaporated and then condensed in the receiving flask. The flame of the burner was kept too close to the bottom of the flask and some of the glucose decomposed into a black carbon deposit on the inside of the flask. During this experiment the following changes occurred. Which of these changes involved a physical change and not a chemical change? formation of a carbon deposit inside the flaskevaporation of ethanolformation of ethanol from glucose by yeastburning of natural gascondensation of ethanolformation of carbon dioxide gas from glucosearrow_forward
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