Question

In: Chemistry

A sample of cooling liquid containing ethylene glycol and water is brought to your lab. The...

A sample of cooling liquid containing ethylene glycol and water is brought to your lab. The cooling tower contains 2,500 tons of this coolant to keep the chillers at an oil refinery working properly. It is critical that the concentration of the ethylene glycol be maintained at a concentration of 44.0±0.5%(w/w), to prevent freezing and transfer the heat properly. Since it’s late and an unexpected cold front has the plant manager worried, you decide to use the refractometer to run this test as fast as possible, yielding a result of 1.3687. Based upon published literature values, does the coolant meet its specification? If not, calculate how much water or ethylene glycol should be added to correct the situation. Would the final volume fill an Olympic-sized pool (660,000 gal)?

The RI indicates its only 36% so I know that part. I'm just not sure on the last two parts of the question.

Solutions

Expert Solution

Knowing that the current concentration of ethylene glycol is only 36%, you can use the following equation to determine the amount of it that is needed:

C1m1 = C2m2

Where C 1 and 2 are concentrations and m 1 and 2 are the corresponding masses.

Now, substitute with the values you already know: (36%)(2500tons) = (44%)(m2)

Now simply solve for the desired mass, getting m2= 3055.55tons. And remember to subtract the previous quantity, to know how much of it there is to add to the current mass, getting then: V= 3055.55 - 2500 = 555.55 tons of ethylene glycol.

From the initial concentration you can know how much water and ethylene glycol you had in the first place:
36% = x / 2500tons, x= 900tons of ethylene glycol and 1600 tons of water.
This also means that you have 900,000 kg of ethylene glycol and 1,600,000 kg of water.

Water has a density of 1 kg /L, from which you can calculate the volume with the equation
1kg/L = 1600000 / v; giving us a volume of 1,600,000 L.

As for ethylene glycol, the density is 1.11kg /L.
1.11kg/L = (900000 + 555555.55 kg) / v; giving us a volume of: 1,311,306.31 L.

And a total volume of: 1,600,000L + 1,311,306.31L = 2,911,306.31 L
Just convert from liters to gallons as:

Then it would be able to fill an olympic pool


Related Solutions

An ethylene glycol solution contains 16.2 g of ethylene glycol (C2H6O2) in 87.4 mL of water....
An ethylene glycol solution contains 16.2 g of ethylene glycol (C2H6O2) in 87.4 mL of water. Part A Calculate the freezing point of the solution. (Assume a density of 1.00 g/mL for water.) Part B Calculate the boiling point of the solution.
An ethylene glycol solution contains 27.6 g of ethylene glycol (C2H6O2) in 90.4 mL of water....
An ethylene glycol solution contains 27.6 g of ethylene glycol (C2H6O2) in 90.4 mL of water. (Assume a density of 1.00 g/mL for water.) Kb of water=0.51C/m and Kf of water=-1.86C/m Part A: Determine the freezing point of the solution. Express your answer in degrees Celsius. Part B: Determine the boiling point of the solution. Express your answer in degrees Celsius.
An ethylene glycol solution contains 29.8 g of ethylene glycol (C2H6O2) in 92.6 mL of water....
An ethylene glycol solution contains 29.8 g of ethylene glycol (C2H6O2) in 92.6 mL of water. (Assume a density of 1.00 g/mL for water.) Part A Determine the freezing point of the solution. Express you answer in degrees Celsius. Part A Determine the freezing point of the solution. Express you answer in degrees Celsius. Part B Determine the boiling point of the solution. Express you answer in degrees Celsius.
An ethylene glycol solution contains 24.6 g of ethylene glycol (C2H6O2) in 89.8 mL of water....
An ethylene glycol solution contains 24.6 g of ethylene glycol (C2H6O2) in 89.8 mL of water. (Assume a density of 1.00 g/mL for water.) a. Determine the freezing point of the solution in degrees Celsius. b. Determine the boiling point of the solution in degrees Celsius.
a 35.0 gram sample of ethylene glycol, is dissolved in 500 grams of water The vapor...
a 35.0 gram sample of ethylene glycol, is dissolved in 500 grams of water The vapor pressure of pure water at 32.0 degrees Celsius at 35.7 torr. what is the vapor pressure of the solution at 32.0 degrees Celsius?
- A 35.0 g sample of ethylene glycol, HOCH2CH2OH is dissolved in 500 g of water....
- A 35.0 g sample of ethylene glycol, HOCH2CH2OH is dissolved in 500 g of water. The vapor pressure of water at 32 C is 35.7 mmHg, What is the vapor pressure of the water/ethylene glycol solution at 32 C? - What is the Boiling Point of the solution resulted from the dissolving of 32.5 g of sugar (C6H12O6) in 250.0 g of water? - . A 1.07 mg sample of a compound was dissolved in 78.1 mg of camphor....
You are given that a 163.5 grams of water and an unknown amount of ethylene glycol...
You are given that a 163.5 grams of water and an unknown amount of ethylene glycol (C2H6O2) were mixed together. The only information given is that the mole fraction of ethylene glycol is .098. Calculate the amount of grams of ethylene glycol as well as the new boiling point and freezing point.
Ethylene glycol, formula C2H6O2, is used as antifreeze for automobiles and is sometimes mixed with water...
Ethylene glycol, formula C2H6O2, is used as antifreeze for automobiles and is sometimes mixed with water at a 1:1 ratio by volume and produces a solution with a density of 1.07 g/mL. Assume that the solution behaves ideally. Notes: at 25 oC the densities of water and ethylene glycol are 1.00 g/mL and 1.11 g/mL, respectively, the vapor pressures of water and ethylene glycol at 20 oC are 17.54 torr and 0.06 torr, respectively, and Kb and Kf of water...
Compare the normal boiling point of ethylene glycol to that of water, and explain any differences...
Compare the normal boiling point of ethylene glycol to that of water, and explain any differences in terms of the intermolecular forces present in each substance.
Ethylene glycol, formula C2H6O2, is used as antifreeze for automobiles and is sometimes mixed with water...
Ethylene glycol, formula C2H6O2, is used as antifreeze for automobiles and is sometimes mixed with water at a 1:1 ratio by volume and produces a solution with a density of 1.07 g/mL. Assume that the solution behaves ideally. Notes: at 25 oC the densities of water and ethylene glycol are 1.00 g/mL and 1.11 g/mL, respectively, the vapor pressures of water and ethylene glycol at 20 oC are 17.54 torr and 0.06 torr, respectively, and Kb and Kf of water...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT