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May 1, 2016

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

Number of results: 45,786

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.
November 28, 2009 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.

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.
January 21, 2011 by Sarah

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 ...

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.
January 31, 2010 by danielle

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?
July 7, 2010 by Linda

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...
February 26, 2010 by Tim

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)
April 27, 2012 by Maggie

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 ...
September 23, 2012 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 -30.0¡ÆC? (The density of ethylene glycol is 1.11 g/cm3, and the density of water is 1.00 g/cm3.)
November 23, 2009 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 -30.0¡ÆC? (The density of ethylene glycol is 1.11 g/cm3, and the density of water is 1.00 g/cm3.)
November 23, 2009 by fdqed

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?
April 10, 2012 by Kelsey

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 -28.0°C? (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 ...
November 30, 2008 by Rita

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 -30.0¡ÆC?
November 23, 2009 by yutyh

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. molality I actually can do this whole problem EXCEPT for one part I'm stuck on. The ...
November 30, 2015 by Kyle

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 ...
January 24, 2009 by Saira

Chemistry
The cooling system in an automobile holds 10.0 L of ethylene glycol antifreeze. How much energy is absorbed when the temperature of the ethylene glycol goes from 20°C to 100°C? The density and specific heat capacity of ethylene glycol are 1.11 g/mL and 2.42 J/(g • °C),
October 21, 2015 by Derek

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
January 18, 2009 by Tanya

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?
June 8, 2010 by Car

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 ...
November 6, 2011 by Monique

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
October 26, 2008 by Gary

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 ...
November 20, 2010 by kai

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 :(
January 24, 2013 by Christine

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?
January 27, 2009 by Agatha

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.
February 2, 2010 by Shanee

Chemistry
How much ethylene glycol (C2H6O2, the major component of antifreeze) must be added to 1 L of water to keep from it freezing at -15 °F?
July 9, 2014 by Anonymous

Chemistry
How much ethylene glycol (C2H6O2, the major component of antifreeze) must be added to 1 L of water to keep it from freezing at -20 oC? Kf = 1.86 oC/m.
February 3, 2015 by Sheila

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...
September 25, 2012 by Holly

Freezing solution
An ethylene glycol solution contains 26.2g of ethylene glycol (C2H6O2) in 81.4mL of water. Calculate the freezing point of the solution. (Assume a density of 1.00 g/mL for water.) how do I set this up?
April 27, 2015 by Chemistry

chemistry
An ethylene glycol solution contains 18.2g of ethylene glycol (C2H6O2) in 85.4mL of water. Calculate the freezing point and boiling point of the solution. (Assume a density of 1.00 g/mL for water.)
November 19, 2014 by Anon

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 ...
April 19, 2010 by Angelica

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.)
May 21, 2011 by Sara

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
October 27, 2010 by Tara

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 ?
August 15, 2013 by ethelyn

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?
March 15, 2010 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?
March 15, 2010 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?
March 15, 2010 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?
March 16, 2010 by Katelynn

Chemisty
Antifreeze is made by mixing equal volumes of ethylene glycol (d=1.114 g/mL) and water. The resulting solution has a density of 1.040 g/mL. Calculate the antifreeze molarity, molality, mole fraction, mass percent, and volume percent.
December 6, 2015 by Anonymous

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?
November 22, 2011 by Mathieu

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 ...
February 27, 2011 by dylan

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
June 21, 2013 by Katie

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
February 11, 2009 by Danielle

Chemistry
The vapor pressure of water at 25°C 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 ...
January 26, 2011 by Rukky

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
March 22, 2011 by Lilly

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 ...
January 25, 2009 by Dr Bob plz conform

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?
February 8, 2013 by kylie

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 ...
January 20, 2010 by bubble

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...
March 24, 2007 by Jakob

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 ...
February 15, 2013 by K

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?
March 8, 2012 by teetee

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 ...

chemistry
The vapor pressure of pure water at 70°C 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 ...

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 -23.3°C. Assume the density for water is exactly 1 g/m.L
January 27, 2009 by -

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
November 5, 2011 by Monique

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...
July 11, 2011 by determining molar mass

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 ...
January 25, 2009 by Writeacher

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 ...
October 18, 2010 by Stacey

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 32.5°C (c of ethylene glycol = 2.42 J/gK)? Please help me, I don't even know where to begin!!
October 18, 2010 by Megan

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.
September 13, 2010 by MW

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 32.5°C (c of ethylene glycol = 2.42 J/gK)?
October 19, 2010 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 32.5°C (c of ethylene glycol = 2.42 J/gK)?
October 20, 2010 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 32.5°C (c of ethylene glycol = 2.42 J/gK)?
October 18, 2013 by Anonymous

chemestry
27.2 g sample of ethylene glycol, a car radiator coolant, loses 685 J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5°C (c of ethylene glycol = 2.42 J/gK)?
October 23, 2015 by mara

chemistry
calculate the mole fraction of ethylene glycol in a solution containing 20% of ethylene glycol prepared in water. answer it as fast as possible.........
August 2, 2015 by raksha

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.
January 27, 2009 by Raj

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

Chemistry
A 50.0mL sample of ethylene glycol had a mass of 55.505g. Find the density of ethylene glycol.
September 19, 2011 by jess

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?
October 5, 2008 by Anna

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? ...
April 29, 2012 by Jen

Algebra
One type of anyifreeze is 40% glycol, and another type of antifreeze is 60% glycol. How much of each kind should be used to make 100 gallons of antifreeze that is 48% glycol? How do i show my work? Thanks
November 8, 2015 by Gabe

chemistry
A 49.3 g sample of ethylene glycol, a car radiator coolant, loses 624. J of heat. What was the initial temperature of ethylene glycol if the final temperature is 32.5°C (c of ethylene glycol = 2.42 J/gK)? 624= 49.3 x 2.42(T-32.50) T = 37.73 = 38degrees is this correct? thank ...
October 13, 2015 by patrick

chem
An ethylene glycol solution contains 21.5 of ethylene glycol in 82.9 of water.
February 19, 2013 by Anonymous

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?
January 19, 2013 by caran

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?
September 27, 2012 by Thy

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 ...
January 22, 2009 by Saira

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

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.
March 13, 2011 by Emilene

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 25°C?
February 10, 2013 by Marcus

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?
February 12, 2013 by jenny

chemistry
1.00 of an aqueous solution contains 1.52g of a compound used in antifreeze. If the osmotic pressure of this solution at 20.0 degree C is 448 torr, calculate the molar mass of the antifreeze compound
April 28, 2014 by courtney

Chemistry
Determine the vapor pressure (in atm) of water in an aqueous solution of 12% by mass ethylene group (antifreeze) if the vapor pressure of pure water at that temperature is 0.095 atmospheres.
February 15, 2016 by Samantha

Chemistry
The density of a 22.0% by mass ethylene glycol (C2 H6 O2) solution in water is 1.03 .Find the molarity of the solution.
February 11, 2009 by HELP PLEASEEE

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.
August 3, 2011 by eddy

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!
December 4, 2010 by Julie

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.
October 4, 2010 by jerry

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.
August 4, 2008 by Jared

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 0.0ºC and Kf of pure water is -1.86ºC/m.
August 21, 2010 by Cecilia

Chem 132
If the density of a 40.0 mass % solution of ethylene glycol in water is 1.0514g/mL at 20 celcius what is the molarity
September 24, 2014 by RB

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.
February 14, 2011 by redgy

chemistry
A 35.0g sample of ethylene glycol is dissolved in 500.0g of water. The vapor pressure of water at 32C is equal to 35.7mm Hg. What is the vapor pressure of the water-ethylene glycol solution at 32C?
August 24, 2014 by jojo

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 ...
October 8, 2010 by lucylu

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)
June 10, 2012 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)
June 10, 2012 by Verls

Chemistry
Ethylene glycol has a specific heat of 0.578 cal/(g×°C). If 23.2 g of ethylene glycol absorbs 75.6 cal of heat energy, what will the temperature increase be?
November 29, 2011 by Chemistry Chick

chemistry
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 1.86C kg) what i tried was 18/62 to find the moles. then i got .29/.150 to solve for the molality. then i ...
April 7, 2008 by david

chemistry
the density of water 20 degrees celcius is 1.00g?mL and the densityof ethylene glycol is 1.114g/mL, if 100.0mL if water is combined with 25.0mL is ethylene glycol, what would be the density of this mixture?
October 17, 2012 by mat

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...
April 12, 2008 by mia

chemistry
why would it not be useful to just use pure ethanil or pure ethylene glycol as aN ANTIFREEZE SINCE THEIR NORMAL FREEZING POINTS are -114.1 degrees celsius and -12 degrees celsius respectively
February 8, 2011 by shaknocka lewis

chemistry
why would it not be useful to just use pure ethanil or pure ethylene glycol as aN ANTIFREEZE SINCE THEIR NORMAL FREEZING POINTS are -114.1 degrees celsius and -12 degrees celsius respectively
February 8, 2011 by shaknocka lewis

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