?3?6 + 1.5?2 → ?3?4?2 + ?2O. Annual production rate of acrylic acid is 8206576 kg/year. Assume your reaction has 90% conversion, 65% yield, and oxygen is supplied by air fed50% in excess. Complete the mass balance for your product. Summarize your results in 2 tables: a mole balance table and a mass balance in a table. Put these tables in the executive summary What is the mass balance?

How to apply process parameter of flow of HAZOP on a dishwasher, washing machine, lawn mower, car, or vacuum cleaner?

Question 1

A calorimeter is a device which can be used to determine the heat of reaction. The process of measuring the heat is known as calorimetry. Based on the above statement and from your further findings, answer the following questions:

a) Analyze the operational principle of a calorimeter in a proper sequence. Organize your answer in the form of a flow diagram :

b) Outline how does the operational principle of the calorimeter is related to the First Law of Thermodynamics.

Question 2

Electroplating is a process of passing through an electrical current through an electrolyte solution, which the intention to change the surface properties of an object; such as corrosion protection, abrasion/wear resistance and aesthetic qualities. Electoplating has been widely used in jewelry making, which can enhanced the aesthetic value and its wearability. Based on the electroplating process in jewelry making, answer the following questions:

a) Identify one (1) type of material which can be used for the jewelry electroplating.

b) Sketch the diagram of the electrolysis cell (based on the material selected in a). The sketch must be hand-drawn, without any copy and paste from any source.

c) Analyze all the reactions involve in the process (half cell reactions and overall cell reaction).

d) Identify the oxidizing agent and reducing agent. Provide the reason(s) for the identification.

e) Analyze the limitation or constraint of this process.

100mL of 3M NaOH is poured into 100mL of 3M HF. The highest temperature reached is 48.71 degrees Celcius.

3M NaOH inital temp= 25 degrees Celcius

3M HF inital temp= 25 degrees Celcius

a. How many moles of Hf reacted? How many moles of NaOH?)

b. Assuming the specific heat of the mixed solution is 4.18 J/(g*C), and that the density of the mixed solution is 1.00 g/mL, use q = CDT to determine the heat added to the solution.

c. Heat evolved by the reaction is the negative of heat added to the solution. Find heat evolved per mol of HF that reacts.

d. Compare the %deviation of the result of c. to the result of Part 1 for this reaction.

Does the highest temperature reached (48.71) show accurate heats of reaction?

A fuel gas containing an equimolar (equal molar amounts) mixture of propane and carbon disulfide is burned completely with 32% excess air.

Assume a 100 mol propane/s basis of calculation. If the fuel enters the process at 187 ^oC and 120 atm calculate the volumetric flow rate (L/s) of the entering gas. Do not assume the gas is ideal.

a) Write the balanced chemical reaction(s) for the fuel.

b) Determine the rate (mol/s) air is fed to the furnace.

c) Calculate the total flowrate (mol/s) of the mixture leaving the reactor.

d) Calculate the mole fraction of oxygen in the product gas.

e) Calculate the mole fraction of carbon dioxide in the product gas.

Give 5 pros of Corrosion

and give 5 cons of Corrosion on how to solve this problem

Three objects, cylindrical rod (radius = 0.1 m), steel ball (radius = 0.1 m) and flat screen (length = 0.1 m) with surface temperature of 65 ℃ are exposed in perpendicular direction to water flow at 30 m/s and 30 ℃. Assume the area of all three objects are the same as 1 m2 , determine the individual values of convective heat transfer coefficient for each object, and their respective heat loss.

Depending on the sample of interest, different ion sources are used for mass spectrometry. What ion source would you use if you wanted to examine many different small molecules and compare your results to a large database? Why?

6.8 Raw natural gas flowing at 1000 mol/h contains 15.0 mol% CO₂,5.00 mol% H₂S, and 1.41 mol% COS, and the balance is methane.The separations system shown in Problem Figure 6.8.1 is capable of handling a certain flow rate of raw natural gas. Any flow rate higher than this limit is sent into the bypass around the separation unit and then mixed with the treated gas to yield the final product. The final product is to contain no more than 1.00 mol% H₂S and no more than 0.300 mol% COS. Stream 6 leaving the separation unit contains H2S and COS only. The separations unit maximum flow rate it can handle is 900 mol/h; any flow beyond this must go to the bypass system. Find out the flow rate of the treated natural gas stream and flow rate of the reject stream from the separator? (948.2, 51.8 mol/h)

A solvent-extraction process usingN,N − diethyldodecanamide, which is insoluble in water and has a density of 0.847 g / cm3 . In a typical experiment at 30°C, 50 g of 20 wt % citric acid and 80 wt % water was contacted with 0.85 g of amide. The resulting organic phase, assumed to be in equilibrium with the aqueous phase, contained 6.39 wt % citric acid and 2.97 wt % water. Determine the partition (distribution) coefficients for citric acid and water

a) How to identify the smoke filling time?

b) What are the factors affecting the minimum intensity of radiative flux ?

Explain how ultra-rapid cooling of some metal alloys produces metallic glass.

STEPS:

Part III – Copper Charge

18. Measure and record the mass of a clean, dry crucible with its cover. Record this value to within 0.001 g.

19. Obtain and record the copper chloride hydrate mass.

a. Obtain about one gram (1 ± 0.1 g) of the unknown copper chloride hydrate using a weigh paper.

b. Place the unknown copper chloride in the crucible. Use a spatula to carefully break up any large pieces of the substance by pressing the pieces against the wall of the crucible.

c. Measure and record the mass of the crucible with the compound. Record your data to within 0.001 g.

20. Hold the burner in your hand and move the flame slowly back and forth underneath the crucible to gently heat the sample. Do not overheat the compound! The sample will make a popping noise and stick to the bottom of the crucible if overheated. Record anything that is observed during heating.

21. Once heating is completed, turn off the equipment and allow the sample to cool.

22. Remove the crucible cover and carefully inspect the sample. If any of the sample has maintained its initial appearance, reheat the sample until all of it has reacted.

23. Measure and record the mass of the cool crucible, lid, and dry (anhydrous) copper chloride sample. Record this mass to within 0.001g

24. Generate a solution of the copper chloride.

a. Transfer the brown solid to a clean and empty 50 mL beaker. Rinse out the crucible with two 8 mL aliquots (measured portions of a liquid) of deionized water and pour the water into the 50 mL beaker.

b. Gently swirl the beaker or stir the solution with a glass stir rod to completely dissolve the solid. Record any observations, particularly color change.

25. React the copper chloride solution to generate elemental copper.

a. Obtain a piece of aluminum wire. If the wire is dull, sand it with the sandpaper until shiny.

b. Coil the wire loosely around your index and middle fingers. Fewer coils are better.

c. Place the wire in the beaker of copper chloride solution so that it is completely immersed. It may need to be pushed down with a stir rod. Make sure the reaction goes to completion before continuing.

26. Complete the reaction.

a. Add 5 drops of 6 M HCl solution to dissolve any aluminum salts in the mixture, leaving a clear solution.

b. Use a glass stir rod to scrape off the copper from the aluminum wire into the beaker. Remove the aluminum wire from the solution and rinse it with deionized water or 1-2 drops of HCl to remove any additional copper.

c. Once the aluminum wire is rinsed, place the wire aside on a Kimwipe.

27. Collect and wash the copper produced in the reaction.

a. Set up a Büchner funnel for vacuum filtration.

b. Isolate the copper with the filter and rinse it with some deionized water.

c. Break up any large pieces of copper and rinse it twice with small amounts of deionized water.

d. Turn off the suction on the vacuum filtration apparatus.

a. Measure and record the mass of a clean, dry watch glass. Record this mass to within 0.001 g.

b. Remove the filter from the Büchner funnel and transfer the copper to the watch glass. Try to disperse the copper evenly on the watch glass.

c. Dry the watch glass with copper in an oven for 10-15 minutes.

d. Remove the watch glass using crucible tongs and let the watch glass cool.

e. When it is cool enough to touch, measure the mass of the watch glass and copper. Record this mass to within 0.001 g.

28. Dry the copper sample and take mass measurements.

29. Repeat drying in the oven and weighing the copper until the last two mass measurements are within 0.005 g of each other.

1. From the mass of copper measured in Part III, determine the moles of Cu.

Mass of crucible with cover was 37.111 g. Mass of copper chloride hydrate 38.066g total (0.958g of copper chloride hydrate). Mass of (anhydrous) copper chloride sample 37.857g (w/ crucible). Dry copper mass with watch glass (recorded 3 times after putting back in the oven) is 37.195g, 37.189g and 37.188g. The weight of the watch glass was 36.828g.

2. Determine the mass of chlorine in the original sample as the difference in mass between the anhydrous sample (after drying in the crucible) and the mass of copper. From the mass of chlorine, determine the moles of Cl.

3. Determine the experimental molar ratio of Cu:Cl.

4. In Step 26, describe the components involved in the reaction. What evidence is there for a chemical reaction? Describe where the reaction is occurring on the molecular level.

26) Complete the reaction.

a. Add 5 drops of 6 M HCl solution to dissolve any aluminum salts in the mixture, leaving a clear solution.

b. Use a glass stir rod to scrape off the copper from the aluminum wire into the beaker. Remove the aluminum wire from the solution and rinse it with deionized water or 1-2 drops of HCl to remove any additional copper.

c. Once the aluminum wire is rinsed, place the wire aside on a Kimwipe.

5)

a. Without attempting to measure the mass of the aluminum wire, consider the reaction that occurs in step 26, what would an increase in the metal wire mass indicate?

b. What would a decrease in the metal wire mass indicate?

Which standard sets limits on effluent water quality of an industrial facility?

(i) Water quality objective limits (ii) Discharge standard (iii) Primary drinking water standard (iv) Secondary drinking water standard

A shell-and-tube heat exchanger with two tube passes and baffled single shell pass is used as oil cooler. Cooling water at 20°C flows through the tubes at a flow rate of 4.082 kg/s. Engine oil enters the shell side at a flow rate of 10 kg/s. The inlet and outlet temperatures of oil are 90°C and 60°C, respectively. The overall heat transfer coefficient based on the outside tube area (U_o) is 262 W/m²⋅K. The specific heats of water and oil are 4.179 kJ/kg⋅ ^oC and 2.118 kJ/kg⋅ ^oC, respectively.

Calculate:

1. Heat Duty Q (kW) and cooling water outlet temperature
2. The corrected log mean temperature difference
3. The surface area of the heat exchanger using the LMTD
4. The effectiveness of the heat exchanger (ε) and capacity ratio (c)
5. The number of transfer units (NTU)