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Search: An aqueous antifreeze solution is 40.0% ethylene glycol (C2H6O2) by mass

Number of results: 40,805

Chemistry
An aqueous antifreeze solution is 40.0% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.05 g/cm3. Calculate the molality, molarity, and mole fraction of the ethylene glycol.
Friday, January 21, 2011 at 11:33am by Sarah

AP Chemistry
An aqueous antifreeze is 40.0% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.05 g/cm3. Calculate the molality, molarity, and mole fraction of the ethylene glycol.
Saturday, November 28, 2009 at 2:34pm by Angel

Chemistry
An aqueous antifreeze solution is 31.0% ethylene glycol (C2H6O2) by mass. The density of the solution is 1.039 g/cm3. Calculate the molality of the ethylene glycol.
Thursday, March 14, 2013 at 3:57pm by Maddie

chemistry
I need help solving this question.. An aqueous solution of ethylene glycol (C2H6O2) IS 40% ethylene glycol by mass, and has a density of 1.05g/ml. what are the molarity, molality fraction of the solution?
Wednesday, July 7, 2010 at 10:20pm by Linda

Chemistry
3) The chemical formula for ethylene glycol (antifreeze) is C2H6O2 and Isopropyle alcohol is C3H7OH. Calculate the new boining and freezing oints for 1000.0 g of aqueous solution (total volume), that is 30.0% solute (the antifreeze and the alcohol are the solutes). You will ...
Thursday, May 19, 2011 at 10:25am by Adam

chemistry
Automotive antifreeze consists of ethylene glycol, C2H6O2, a nonvolatile electrolyte. Calculate the boiling point and freezing point of a 25.0 mass percent of ethylene glycol in solution.
Sunday, January 31, 2010 at 11:26pm by danielle

chemistry
Ethylene glycol, C2H6O2, is used as antifreeze for automobile engines. If you want to produce 2.00 kg of ethylene glycol from the reaction of C2H4Cl2 and Na2CO3, what is the minimum amount of Na2CO3 that is needed? C2H4Cl2(l) + Na2CO3(s) + H2O(l)=C2H6O2(l) + 2NaCl(aq) + CO2(g)
Friday, April 27, 2012 at 12:25am by Maggie

Chemistry.
What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 13.7 L of water to produce an antifreeze solution with a freezing point of -30.0C? (The density of ethylene glycol is 1.11 g/cm3, and the density of water is 1.00 g/cm3.)
Monday, November 23, 2009 at 3:06pm by ?

Chemistry
What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 13.7 L of water to produce an antifreeze solution with a freezing point of -30.0C? (The density of ethylene glycol is 1.11 g/cm3, and the density of water is 1.00 g/cm3.)
Monday, November 23, 2009 at 11:42pm by fdqed

chemistry
What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 20.0 L of water to produce an antifreeze solution with a freezing point of -28.0C? (The density of ethylene glycol is 1.11 g/cm3, and the density of water is 1.00 g/cm3.) .....L What is the boiling ...
Sunday, November 30, 2008 at 12:54pm by Rita

chemistry
Calculate the vapor pressure of water over each of the following ethylene glycol C2H6O2 solutions at 80 degree C (vp=pure water=657.6 mm Hg). Ethylene glycol can be assumed to be nonvolatile. (a) X (ethylene glycol)= 0.288 (b) % ethylene glycol by mass =39% (c) 2.42 m ethylene...
Friday, February 26, 2010 at 6:46pm by Tim

Chemistry
I need help ASAP! Colligative Properties- Ethylene glycol (C2H6O2) is the principal ingredient in antifreeze. How many grams of ethylene glycol will be needed to lower the freezing point of 2100 grams of water by 20 degrees celcius?
Tuesday, April 10, 2012 at 10:36pm by Kelsey

Chemistry
What is a minimum volume (in gallons) of ethylene glycol (CH2OHCH2OH, an antifreeze) that has to be added to 3.00 gal of water if you desire this engine cooling solution (for a auto radiator) NOT to be frozen below - 34.1 oC - a very cold Siberian or Canadian winter ...
Sunday, September 23, 2012 at 8:53pm by E. Lee

chemistry
What volume of ethylene glycol (C2H6O2), a nonelectrolyte, must be added to 13.7 L of water to produce an antifreeze solution with a freezing point of -30.0C?
Monday, November 23, 2009 at 11:41pm by yutyh

College Chemestry
an agueous solution of ethlylene glycol (C2H6O2) is 40% ethylene glycol by mass, and has a density of 1.05g/ml. What are the molarity, molality, and mole fraction of the solution? Do you know how to solve this...I am kinda lost..please help
Sunday, October 26, 2008 at 7:38pm by Gary

chemistry
A 13.03 g sample contains only ethylene glycol (C2H6O2) and propylene glycol (C3H8O2). When the sample is added to 100.0g of pure water, the resulting solution has a freezing point of -3.5C. What is the percent composition of ethylene glycol and propylene glycol in the ...
Sunday, November 6, 2011 at 9:41pm by Monique

physics
an antifreeze solution is made by mixing ethylene glycol (density= 1116 kg/m^3) with water. suppose that the specific gravity of such a solution is 1.0730. assuming that the total volume of the solution is the sum of its parts, determine the volume percentage of ethylene ...
Saturday, November 20, 2010 at 11:33pm by kai

Chemistry
I need this answered really fast. 4. Ethylene glycol (C2H6O2) is used as an antifreeze in cars. If 400 g of ethylene glycol is added to 4.00 kg of water, what is the molality? Calculate how much the freezing point of water will be lowered. The freezing-point depression ...
Friday, May 17, 2013 at 4:45pm by Lauren

Chemistry
The antifreeze in a car is a 50% by weight solution of ethylene glycol, C2H6O2 in a water solvent. Calculate the boiling point and freezing point of this solution. (For H2O, Kb=0.52 C/m Kf= 1.86 C/m I can't even find the formula for this in my book, please help :(
Thursday, January 24, 2013 at 7:13pm by Christine

CHM 152
An automobile antifreeze contains equal volumes of ethylene glycol (d=1.114 g/mL and FW = 62.07) and water (d=1.00 g/mL) at 25oC. The solution has a density of 1.06 g/mL. What is the molarity of ethylene glycol in the solution?
Tuesday, June 8, 2010 at 12:06am by Car

chem
An ethylene glycol solution contains 23.9 g of ethylene glycol (C2H6O2) in 86.9 mL of water. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)
Saturday, May 21, 2011 at 9:12am by Sara

Chemistry
What mass of ethylene glycol C2H6O2, the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23.3 degrees Celsius? Assume the density for water is exactly 1 g/mL
Sunday, January 18, 2009 at 7:47pm by Tanya

chemistry
what is the molarity of an antifreeze solution glycol in water containing 15.4 g of ethylene glycol (HOCH2CH2OH) and 84.6 g H2O ?
Thursday, August 15, 2013 at 10:42am by ethelyn

chemistry
Ethylene glycol (antifreeze) has a specific heat of 2.42 J/(g*K). Calculate q when 3.65 kg of ethylene glycol cools from 240 degrees C to 78 C
Wednesday, October 27, 2010 at 1:18pm by Tara

chemistry
What is the boiling point of the water in your radiator if 2.00kg of antifreeze (ethylene glycol, C2H6O2) is added to 9.00x10^3 grams of water?
Monday, March 15, 2010 at 10:24pm by Katelynn

chemistry
What is the boiling point of the water in your radiator if 2.00kg of antifreeze (ethylene glycol, C2H6O2) is added to 9.00x10^3 grams of water?
Monday, March 15, 2010 at 10:29pm by Katelynn

chemistry
What is the boiling point of the water in your radiator if 2.00kg of antifreeze (ethylene glycol, C2H6O2) is added to 9.00x10^3 grams of water?
Monday, March 15, 2010 at 10:30pm by Katelynn

chemistry
What is the boiling point of the water in your radiator if 2.00kg of antifreeze (ethylene glycol, C2H6O2) is added to 9.00x10^3 grams of water?
Tuesday, March 16, 2010 at 6:08pm by Katelynn

Chemistry
A popular brand of automobile radiator antifreeze advertises that their product (ethylene glycol; C2H6O2) provides engine protection from temperatures of -64C to 135C when mixed with water in a 50%/50% mix. What is the boiling point elevation and freezing point depression ...
Monday, April 19, 2010 at 12:36am by Angelica

chemistyr
How much ethylene glycol (C2H6O2, the major component of antifreeze) must be added to 1 L of water to keep it from freezing at -16 oC?Kf = 1.86 oC/m.
Tuesday, February 2, 2010 at 11:15am by Shanee

Chemistry: molality and freezing point?
What mass of ethylene glycol C2H6O2, the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23.3C? Assume the density for water is exactly 1g/mL. m = moles solute / kg solvent Help please?
Tuesday, January 27, 2009 at 10:53pm by Agatha

Math
A chemist has two ethylene glycol and water solutions: one that contains 11.98% ethylene glycol and another with 7.30% ethylene glycol. How many litres of each must be mixed to make 7.50 x 102 L containing 10.50% ethylene glycol?
Tuesday, November 22, 2011 at 10:28pm by Mathieu

CHemistry....Please double check DrBobb
What mass of ethylene glycol C2H6O2, the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23C? Assume density for water is exactly 1g/mL. First we find out the freezing point: =(-23.0)-(0.0_ =-23.0 ...
Saturday, January 24, 2009 at 1:06pm by Saira

Chem
An ethylene glycol solution contains 20.9 g of ethylene glycol (C2H6O2) in 85.0 mL of water. Compute the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.) freezing point C boiling point C How would I set this up? thanks
Tuesday, March 22, 2011 at 6:53pm by Lilly

Chemistry
I've got a similar question as a previous student. What is a minimum volume (in gallons) of ethylene glycol (CH2OHCH2OH, an antifreeze) that has to be added to 3.00 gal of water if you desire this engine cooling solution (for a auto radiator) NOT to be frozen below - 25.9 oC...
Tuesday, September 25, 2012 at 12:30am by Holly

Chemistry
For the ethylene glycol solution. The density is 1.03 g/mL. How much will a liter of the solution weigh? That will be 1.03 g/mL x 1000 mL = 1030 grams. How much of that is ethylene glycol. 22%? So how much with the ethylene glycol weigh? That will be 1030 x 0.22 = ?? How many ...
Wednesday, February 11, 2009 at 7:22pm by DrBob222

chemistry
I don't know what you mean by molality fraction. mass of 1,000 mL = 1.05 g/mL x 1000 = 1050 gram. That is 40% ethylene glycol; therefore, 1050 x 0.40 = 420 g ethylene glycol and 420 g is 420/molar mass ethylene glycol. That will give you moles/L which is M. To find molality, ...
Wednesday, July 7, 2010 at 10:20pm by DrBob222

Chemistry
The vapor pressure of water at 25C is 23.76 mm Hg. What would you calculate as the new vapor pressure of a solution made by adding 50.5 g of ethylene glycol (HOCH2CH2OH, antifreeze) to 50.5 g of water? You may assume that the vapor pressure of ethylene glycol at this ...
Wednesday, January 26, 2011 at 2:46pm by Rukky

Chemistry
The density of a 22.0% by mass ethylene glycol (C2H6O2) solution in water is 1.03 g/mL. Find the molarity of the solution. Answer in M
Wednesday, February 11, 2009 at 7:22pm by Danielle

Chemistry
Antifreeze (commonly ethylene glycol or propylene glycol) is usually mixed with water in the radiator of a car. What is its function and how does it work?
Thursday, March 8, 2012 at 5:18am by teetee

chemistry
The vapor pressure of pure water at 70C is 231 mm Hg. What is the vapor pressure depression of a solution of 115 g of the antifreeze ethylene glycol, C2H6O2, a nonvolatile compound, in 205 g of water? Use molar masses with at least as many significant figures as the data ...
Wednesday, December 12, 2012 at 6:20pm by Brad

chem
An ethylene glycol solution contains 21.5 of ethylene glycol in 82.9 of water.
Tuesday, February 19, 2013 at 4:35pm by Anonymous

Chemistry
A 26.7 g sample of ethylene glycol, a car radiator coolant, loses 668 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5C (c of ethylene glycol = 2.42 J/gK)?
Tuesday, October 19, 2010 at 11:48pm by Brittany

Chemistry
A 26.7 g sample of ethylene glycol, a car radiator coolant, loses 668 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5C (c of ethylene glycol = 2.42 J/gK)?
Wednesday, October 20, 2010 at 1:52pm by Brittany

chem
A 28.9 g sample of ethylene glycol, a car radiator coolant, loses 689 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5C (c of ethylene glycol = 2.42 J/gK)?
Friday, October 18, 2013 at 11:02pm by Anonymous

ap chem
ok, i'm given: Ethylene Glycol C2H6O2 is the main ingredient in antifreeze. density of pure EG: 1.132 g/mL Anti-freeze is 32% by volume EG I have to find: Volume of Eg in 1 L Mass of Eg in 1 L & the Volume of "solvent" in 1 L Can someone help me? and give me some tips? For ...
Sunday, February 27, 2011 at 2:28am by dylan

Chemistry
A 26.5 g sample of ethylene glycol, a car radiator coolant, loses 675 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5C (c of ethylene glycol = 2.42 J/gK)? Please help me, I don't even know where to begin!!
Monday, October 18, 2010 at 10:35am by Megan

chemistry
An ethylene glycol solution is mad using 58.5g of (C2H6O2) and diluting to a total volume of 500.0 mL. Calculate the freezing and boiling point. Assume a density of 1.09 g/ml for the solution
Saturday, November 5, 2011 at 9:49am by Monique

Chem
a) An ethylene glycol solution contains 21.1 g of ethylene glycol in 86.0 ml of water. compute the freezing point of the solution. b) Compute the boiling point of the solution.
Sunday, March 13, 2011 at 5:53pm by Emilene

Chemistry
Can someone please explain this to me?! Please! Thank you! How much (in kilograms) ethylene glycol antifreeze (C2H6O2)(molar mass 62.02 g/mol) has to be added to 14.4 kg of water to get a mixture that freezes at -15.5 degrees C. For water Kf = 1.86 degrees C kg/mol
Friday, June 21, 2013 at 8:45pm by Katie

Chemistry
I need help setting up this problem: Ethylene glycol has a specific gravity of 1.1088 at room temperature, What is the volume of 1.00 kg of ethylene glycol? What is the volume of 2.00 lb of ethylene glycol? Using 25 degrees Celsius.
Monday, September 13, 2010 at 10:17pm by MW

Chemistry
Chemistry - Danielle , Wednesday, February 11, 2009 at 7:24pm The density of a 22.0% by mass ethylene glycol (C2H6O2) solution in water is 1.03 g/mL. Find the molarity of the solution. Answer in M
Wednesday, February 11, 2009 at 7:25pm by Danielle

Chemistry
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d=1.114 g/mL; M=62.07 g/mL) and water (d=1.00 g/mL) at 20 degrees C. The density of the mixture is 1.070 g/mL. Expreess the concentration of ethylene glycol as volume percent. I've tried this ...
Monday, October 18, 2010 at 3:58pm by Stacey

chemistry
A 115 mL sample of a 10.0 M ethylene glycol (C2H6O2) solution is diluted to 1.30 L. What is the freezing point of the final solution? (Assume a density of 1.06 g/mL for the final solution.) What is the boiling point of the final solution? How would I go about setting this up? ...
Sunday, April 29, 2012 at 1:09am by Jen

confused
as i earlier posted and , 1 day ago , i am confusesd hw we ll find freezing point......isnt it T pure solvent - T solution .. which ll be 0-(-23.3) = 23.3 plz conform .. and do we have to use Kf.m .. formula in order to get ( -23.3)(1)= -23.3 .. as someone earlier posted plz ...
Sunday, January 25, 2009 at 12:27pm by Dr Bob plz conform

Chemistry
40% means 40 g ethylene glycol/100 g solution. 40 g to moles = 40/molar mass. Use density to convert 100 g soln to volume, then M = moles/L. Convert % to m 40g/100 g = 40g glycol/(40g glycol + 60 g water). Convert 40 g glycol to moles. Convert 60 g water to kg. m = moles/kg ...
Friday, January 21, 2011 at 11:33am by DrBob222

chemistry
Calculate the normal freezing point of an aqueous solution containing 30% w/w ethylene glycol. Thanks
Wednesday, October 26, 2011 at 10:00pm by el

Science
I need to calcuted the molarity from this 12.5 g of ethylene glycol antifreeze dissolved in o.100kg of water. Density of solution is 1.0 g/mL I know molarity if mole of solute / L of solution. I am confused on how to find the L of solution. Do I add 12.5 and .100g to get the ...
Friday, February 15, 2013 at 9:55pm by K

CHEMISTRY!
what mass of ethylene glycol C2H6O2 the main component of anitfreeze, must be added to 10.0L water to produce a solution for use in a car's radiator that freezes at -23.3C. Assume the density for water is exactly 1 g/m.L
Tuesday, January 27, 2009 at 7:20pm by -

Chemistry repost
Whoever you are -- Please DO NOT USE TUTORS' NAMES where your name or nickname should be. ~~~~~~~~~~~~~~~~~~~~~~~~~~ as i earlier posted and , 1 day ago , i am confusesd hw we ll find freezing point......isnt it T pure solvent - T solution .. which ll be 0-(-23.3) = 23.3 plz ...
Sunday, January 25, 2009 at 6:00pm by Writeacher

CHM 152
1.06 g/mL x 1000 = 1060g is mass 1000 mL soln. This 1000 mL soln consists of 500 mL ethylene glycol and 500 mL H2O(equal volumes of ethylene glycol and H2O). The mass of 500 mL ethylene glycol is 500 x 1.114 g/mL = 557 grams or 557/62.07 = 8.97 moles ethylene glycol per 1000 ...
Tuesday, June 8, 2010 at 12:06am by DrBob222

chemistry
1)If 746.4 g of a substance is dissolved in 1723 g of benzene solvent, the freezing point of the solution is -9.19 oC. Calculate the apparent molar mass (g/mol) of substance. 2) What mass ( g ) of the solvent water should be mixed with 0.008595 L of the solute ethylene glycol ...
Wednesday, January 20, 2010 at 1:14am by bubble

Chemistry
I could add ethylene glycol (antifreeze). I would not think of ethene being a precursor of octane.
Friday, October 12, 2012 at 8:54pm by DrBob222

chemistry
Ethylene glycol (antifreeze) has a density of 1.11 {\rm g/cm^3}.What is the mass in G of 435mL of this liquid?
Friday, February 8, 2013 at 4:41pm by kylie

chemistry
Ethylene glycol (antifreeze) has a density of 1.11 g/cm^3 What is the volume in liters of 3.42 kg of this liquid?
Saturday, January 19, 2013 at 10:53am by caran

Chem
I need to calcuted the molarity from this 12.5 g of ethylene glycol antifreeze dissolved in o.100kg of water. Density of solution is 1.0 g/mL I know molarity if mole of solute / L of solution. I am confused on how to find the L of solution. Do I add 12.5 and .100g to get the ...
Friday, February 15, 2013 at 4:12pm by Please please helppppp!!!!!

Chemistry
Is that -20 F? Convert to C. I get approximately -29 but you need to confirm that more accurately. delta T = Kf*m -29 = 1.86*m Solve for m = about 15. m = 15 mol/kg solvent 1 L has a mass of 1 kg; therefore, we need 15 mol ethylene glycol. g ethylene glycol = mols x molar mass...
Monday, July 23, 2012 at 12:17pm by DrBob222

Chemistry
Convert 3.00 gallons H2O to grams. delta T = Kf*m 34.1 = 1.86*m Sole for m. m = mols glycol/kg solvent You have m and kg solvent (from the 3.00 gallons H2O), solve for mols ethylene glycol. mols glycol = grams glycol/molar mass glycol. You know mols and molar mass, solve for ...
Sunday, September 23, 2012 at 8:53pm by DrBob222

CHEM
WHATS IS THE DENSITY OF ETHYLENE GLYCOL IF YOU HAVE A 50ML SAMPLE OF ETHYLENE GLYCOL WITH A MASS OFF 55.505G
Monday, February 7, 2011 at 12:21pm by DENISA

Chemistry
A 50.0mL sample of ethylene glycol had a mass of 55.505g. Find the density of ethylene glycol.
Monday, September 19, 2011 at 9:44am by jess

chem
I am posed with a question which, in order to be solved, needs the Van't Hoff Factor of ethylene glycol. Some research has shown me that ethylene glycol is an electrolyte, but I don't know how it dissociates in water. Any help would be appreciated. It is not an electrolyte and...
Saturday, March 24, 2007 at 4:30pm by Jakob

Chemistry university level
what mass of ethylene glycol, the main component, of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23.3 degree C? Assume the density for water is exactly 1 g/ml.
Tuesday, January 27, 2009 at 7:11pm by Raj

AP Chemistry
A long problem here. You can help by telling me what you don't understand about it before I spent half the night working all of it out in detail. I'll get you started. 40% by mass means 40 g ethylene glycol + 60 g water. Convert 40 g ethylene glycol to moles. moles = grams/...
Saturday, November 28, 2009 at 2:34pm by DrBob222

algebra help please
Mixture Problem... An auto tech needs a radiator to have a 40% antifreeze solution. The radiator currently is filled with 4 gallons of a 25% antifreeze solution. How much of the antifreeze mixture should be drained from the car if the mechanic replaces it with pure antifreeze?
Monday, February 27, 2012 at 1:24pm by kay

Chem II
How many grams of ethylene glycol (C2H6O2) per kilogram of water are needed to give protection up to 120 C in a car radiator?
Tuesday, February 12, 2013 at 12:28am by jenny

chemistry
30% w/w means 30 g ethylene glycol/100 g soln or 30 g ethyl glycol/(30g eth + 70g H2O). Convert 30 g ethylene glycol to moles. moles = grams/molar mass Calculate molality of the solution. That will be molality = moles/kg soln. Then delta T = Kf*m Solve for delta T and subtract...
Wednesday, October 26, 2011 at 10:00pm by DrBob222

Chemistry
I would do this. 5.22m means 5.22 moles in 1 kg solvent. If we take 1 kg solvent we will have 5.22 x molar mass ethylene glycol = 5.22*62 = about 324 g Ethgly. The solution will have a mass of 1000 g + 324 = about 1324 (You need to go through and redo since I've estimated here...
Monday, May 9, 2011 at 11:19pm by DrBob222

chem - freezing point
When 18 g of ethylene glycol C2H6O2 is dissolved in 150 g of pure water, the freezing point of the solution is _____ C. (The freezing point depression constant for water is 186C kgmol.
Monday, October 4, 2010 at 2:19pm by jerry

Chemistry
What is the vapor pressure of a aqueous solution containing 10 % (by weight) ethylene glycol (62 g/mol) at 25 C. PH2O = 24.3 torr at 25C?
Sunday, February 10, 2013 at 6:19am by Marcus

chemistry
Okay so I know how I would normally determine molar mass of a compound *get out periodic table, sum up elements present, eg. H20 = [2(1.008)+16.00]g/mol* But this is for a lab class and they want us to derive it. Info found: Ethylene glycol (C2H6O2 according to book) dissolved...
Monday, July 11, 2011 at 10:39pm by determining molar mass

Chemistry
What is the freezing point of a solution made by dissolving 450 g of ethylene glycol (C2H6O2) in 550 g of water? The freezing point of pure water is 0.0C and Kf of pure water is -1.86C/m.
Saturday, August 21, 2010 at 10:00pm by Cecilia

Chemistry
I am doing a report on ethylene glycol, AKA antifreeze, and I need to figure out if it is naturally occurring or if it is man-made. I can't seem to find this answer anywhere! Please help!
Saturday, December 4, 2010 at 9:00pm by Julie

Chemistry
Ethylene glycol has a specific gravity of 1.1088 at room temperature 25 degrees Celsius. What is the mass of 1.00L of ethylene glycol at this temperature?
Thursday, September 27, 2012 at 11:37am by Thy

Chemistry(Urgent, please help,thank you)
Ethylene glycol does not ionize; remember i is the number of particles. NaCl has two when dissolved in water so i = 2. But ethylene glycol doesn't ionize. You get 6.02E23 particles when you dissolve a mole of ethylene glycol. When you dissolve a mole of NaCl you get 2*6.02E23 ...
Tuesday, February 21, 2012 at 10:45pm by DrBob222

chemistry
When 18 g of ethylene glycol C2H6O2 is dissolved in 150 g of pure water, the freezing point of the solution is ___ (degrees)C. ( The freezing point depression constant for water is 1.86(dgrees)C kg/mol. I know the formulas I just need to see it done step by step please.
Monday, August 4, 2008 at 10:23pm by Jared

CHEM - mole fractions
the vapour pressure of pure water at 110 degrees is 142.7kpa. a solution of ethylene glycol and water has a vapour pressure of 101.3kpa at 110 degrees. assuming that raoults law is obeyed, what is the mole fraction of ethylene glycol in the solution? I get confused when they ...
Friday, October 8, 2010 at 3:47am by lucylu

AP Chem
Combustion of 6.38 mg of ethylene glycol gives 9.06 mg CO2 and 5.58 mg H20. The compound contains only C, H, and O. What are the mass percentages of the elements in ethylene glycol?
Sunday, October 5, 2008 at 6:21pm by Anna

chemistry
Why would it not be useful to just use pure ethanol or pure ethylene glycol as an antifreeze since their normal freezing points are -114.1 C abd -12C respectively.
Monday, February 14, 2011 at 2:10pm by redgy

Chemistry
1. Show quantitatively how you would prepare a solution of 3.10 x 10^2 g of 0.125 molar (m) ethylene alcohol from ethylene glycol and water.
Wednesday, August 3, 2011 at 7:31am by eddy

algebra help please
If he drains x gallons, then .25(4-x) + 1.00x = .40(4) 1 - .25x + x = 1.6 .75x = .6 x = .8 So, after draining .8 gals, he has 3.2 gals of 25% antifreeze. That means he has .8 gals of antifreeze in the radiator. Now he adds .8 gals of pure antifreeze. Then he has 1.6 gals of ...
Monday, February 27, 2012 at 1:24pm by Steve

CHemistry....Please help
What mass of ethylene glycol C2H6O2, the main component of antifreeze, must be added to 10.0 L water to produce a solution for use in a car's radiator that freezes at -23C? Assume density for water is exactly 1g/mL. ----------------------------------- This is what i have so ...
Thursday, January 22, 2009 at 5:16pm by Saira

Chem
If you want to produce 2.00 kg of ethylene glycol from the reaction of C2H4Cl2 and Na2CO3, what is the minimum amount of C2H4Cl2 that is needed? C2H4Cl2(l) + Na2CO3(s) + H2O(l)C2H6O2(l) + 2NaCl(aq) + CO2(g)
Sunday, June 10, 2012 at 10:13am by Verls

Chem
If you want to produce 2.00 kg of ethylene glycol from the reaction of C2H4Cl2 and Na2CO3, what is the minimum amount of C2H4Cl2 that is needed? C2H4Cl2(l) + Na2CO3(s) + H2O(l)C2H6O2(l) + 2NaCl(aq) + CO2(g)
Sunday, June 10, 2012 at 10:14am by Verls

Chem=continued
Can you make up any quantity, then use 175 mL of that solution or must you make up exactly 175 mL. If the former, the procedure I outlined in my previous post will work ok but you will end up using more chemicals than is necessary AND you will have much more solution that is ...
Monday, February 11, 2008 at 3:37am by DrBob222

Chemistry
Ethylene glycol has a specific heat of 0.578 cal/(gװC). If 23.2 g of ethylene glycol absorbs 75.6 cal of heat energy, what will the temperature increase be?
Tuesday, November 29, 2011 at 8:18pm by Chemistry Chick

chemistry
What is the order that these four compounds would travel through a silica gel column during liquid chromatography? a) ethylene glycol, HOCH2CH2OH b) aqueous sodium chloride solution, NaCl (aq) c) propanol, CH3CH2CH2OH d) benzene, C6H6 (eluted first), ???, ???, ???, ??? (eluted...
Saturday, April 12, 2008 at 3:04pm by mia

Chemistry
10% w/w means 10 g ethylene glycol per 100 g solution. mols ethylene glycol = grams/molar mass 10g eth/(90g H2O + 10g eth) mols in 90g H2O = grams/molar mass total mols = mols ethylene glycol + mols H2O Then XH2O = mols H2O/total mols. Psoln = XH2O*PoH2O
Sunday, February 10, 2013 at 6:19am by DrBob222

Chem 2
Convert 2 gallons ethylene glycol to mL then use density to calculate the mass. Convert 2 gallons H2O to mL and use density to calculate the mass. mols ethylene glycol = grams/molar mass molality of the soln then is moles ethylene glycol/kg H2O delta T = 1*Kb*molality. You can...
Saturday, July 14, 2012 at 4:47pm by DrBob222

Chemistry 110, college
mols ethylene glycol = grms/molar mass = ?. Solve for mols. m ethylene glycol = mols/kg solvent Solve for m and substitute into the two equations below. dT = Kf*m and dT = Kb*m
Monday, April 22, 2013 at 2:05pm by DrBob222

Algrbra I
what you have to do is track the amount of solute. If you add up all the smaller amounts, they must total the total amount. Now, 5 gal of a 12% solution contains 5*.12 = .6 gal of solute. Thinking along those lines, 70L of 40% antifreeze contains 28L of antifreeze 70L of 20% ...
Wednesday, February 8, 2012 at 11:42pm by Steve

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