The answer is- Part washers use cleaning solutions that eventually become spent and must be disposed of properly.
Cleaning solutions: Cleaning solution is a liquid solvent or solution used to clean the working surfaces and the parts of a machine.
What type of cleaning solution is Part washers?
- Parts washers are mechanical devices that are designed to be cleaned to remove debris, dirt, oil, paint, and other substances that could potentially contaminate parts to prepare them for assembly, packaging, or even painting.
- They are basically used to clean parts to make them ready for functional use.
- Cleaning solutions for washing used parts are considered a special waste because they can be hazardous waste and are waste from an industrial process.
- Used solvents are almost always hazardous waste. Both solvent and aqueous parts washers produce a sludge that is usually hazardous because it contains toxic metals and solvents from the parts being cleaned.
- Absorbents used to wipe parts after washing are also dangerous if they contain toxic metals in concentrations exceeding regulatory limits or listed hazardous solvents, and used oil may also contain hazardous waste.
- Thus, these cleaning solutions must be disposed of properly.
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Answer:
Explanation:
The molar mass of a given substance corresponds and pertains to the unit mole of the mass substance which is stated in g/mol
no of moles of H = mass of H/molar mass of H
= 2 kg/ 2 g/mol
= 2000 g/ 2 g/mol
= 1000 moles
moles of O2 = mass (O2)/ molar mass (O2)
= 2 kg/ 32 g/mol
= 2000 g / 32 g/mol
= 62.5 moles
Total moles present = (1000 + 62.5) moles
= 1062.5 moles
= 1.063 kmol
Total mass = 2kg + 2kg
= 4 kg
no of moles = mass/molar mass
molar mass = mass/ no of moles
molar mass = 4 kg/ 1.063 kmol
molar mass = 3.763 kg/kmol
The specific volume of the final mixture can be determined by the relation:
![v_{mixture}=\dfrac{ V}{m}](https://tex.z-dn.net/?f=v_%7Bmixture%7D%3D%5Cdfrac%7B%20V%7D%7Bm%7D)
where;
V = 3 m³
m = 4 kg
![v_{mixture}=\dfrac{ 3 \ m^3}{4 \ kg}](https://tex.z-dn.net/?f=v_%7Bmixture%7D%3D%5Cdfrac%7B%203%20%5C%20m%5E3%7D%7B4%20%5C%20kg%7D)
= 0.75 m³/ kg
For the final volume, The molar specific volume is:
![v_M = M_{mixture} *v_{mixture}](https://tex.z-dn.net/?f=v_M%20%3D%20M_%7Bmixture%7D%20%2Av_%7Bmixture%7D)
where;
![M_{mixture} = 3.763](https://tex.z-dn.net/?f=M_%7Bmixture%7D%20%3D%203.763)
![v_{mixture} = 0.75 \ m^3/ kg](https://tex.z-dn.net/?f=v_%7Bmixture%7D%20%3D%20%200.75%20%5C%20%20m%5E3%2F%20kg)
∴
![v_M = 3.763 \ kg/mol \times 0.75 \ m^3/kg](https://tex.z-dn.net/?f=v_M%20%3D%203.763%20%5C%20kg%2Fmol%20%5Ctimes%200.75%20%5C%20m%5E3%2Fkg)
![\mathbf{v_M = 2.82 \ m^3/kmol}](https://tex.z-dn.net/?f=%5Cmathbf%7Bv_M%20%3D%202.82%20%5C%20m%5E3%2Fkmol%7D)
The average atomic mass of hydrogen (99% H-1, 0.8% H-2, and 0.2% H-3) is 1.012 amu.
The average atomic mass of hydrogen can be calculated with the following equation:
![A = m_{H-1}\%_{H-1} + m_{H-2}\%_{H-2} + m_{H-3}\%_{H-3}](https://tex.z-dn.net/?f=%20A%20%3D%20m_%7BH-1%7D%5C%25_%7BH-1%7D%20%2B%20m_%7BH-2%7D%5C%25_%7BH-2%7D%20%2B%20m_%7BH-3%7D%5C%25_%7BH-3%7D%20)
Where:
: is the mass of protium (H-1) = 1
: is the <em>mass</em> of deuterium (H-2) = 2
: is the <em>mass </em>of tritium (H-3) = 3
: is the abundance percent of H-1 = 99%
: is the <em>abundance percent</em> of H-2 = 0.8%
: is the <em>abundance percent</em> of H-3 = 0.2%
The average atomic mass is:
![A = 1*99\% + 2*0.8\% + 3*0.2\%](https://tex.z-dn.net/?f=%20A%20%3D%201%2A99%5C%25%20%2B%202%2A0.8%5C%25%20%2B%203%2A0.2%5C%25%20)
Changing all the <u>percent values</u> into <u>decimal ones</u>, we have:
![A = 0.99 + 2*0.008 + 3*0.002 = 1.012](https://tex.z-dn.net/?f=%20A%20%3D%200.99%20%2B%202%2A0.008%20%2B%203%2A0.002%20%3D%201.012%20)
Therefore, the average atomic mass of hydrogen is 1.012 amu.
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Sodium chloride
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Here we need to see the differences between a liquid and a gas, and how that affects the volume and effects of pressure on them.
The correct option is:
Gases are more readily compressed than liquids are because there is more space between the particles in a gas than in a liquid.
So we have two syringes, one with air and the other with water.
The student applies the same amount of pressure to both of them, but as water is denser than air, in a given change dV of volume in the syringe, the mass of water is larger than the mass of air.
This means that for the same pressure, we should expect the change in volume to be smaller in the syringe with water.
Why this happens?
Gases are more readily compressed than liquids are because there is more space between the particles in a gas than in a liquid.
This means that for the air is easier to be compressed<em> (the distance between particles is larger, so the same pressure compresses more a gas than a liquid)</em> and exit the syringe than for the water, and this translates to the change in volume per unit of pressure applied, <u>which is larger for gases than liquids.</u>
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