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Search: A bottle of wine contains 10.9% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality

Number of results: 96,361

Chemistry
A bottle of wine contains 11.4% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality.
Sunday, September 23, 2012 at 8:55pm by Erin

AP Chemistry
A bottle of wine contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality.
Sunday, November 14, 2010 at 11:56pm by Anonymous

AP CHEMMMM
A bottle of wine contains 13.1% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality. mass percent _______% molality ______mol/kg Thanks
Saturday, November 29, 2008 at 10:22pm by Lawrence

CHEMISTRY MOLALITY!!!!!
A bottle of wine contains 13.1% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality. i don't know how to get molality. please help!!!! Molality is the number of moles of solute ...
Saturday, March 31, 2007 at 10:39pm by Anonymous

Chemistry
In the "Methode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is given below. C6H12O6(aq) 2 C2H5OH(aq) + 2 CO2(g) Fermentation of 712 mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume...
Tuesday, November 13, 2012 at 7:56pm by Zachary

Chemistry
Alcoholic drinks contain ethanol. 10cm3 of ethanol is called one unit of alcohol. Men are advised to drink a maximum of 21 units of ethanol a week, while women are advised to drink a maximum of 14 units. Wine contains about 14% ethanol by volume. A) a bottle of wine contains ...
Saturday, February 8, 2014 at 10:36am by Ella

chem
C6H12O6(aq)->2 C2H5OH(aq) + 2CO2(g) Fermentation of 744mL grape juice(density=1.0 g/cm^3) is allowed to take place in a bottle witha V of 825mL until 12% by volume is ethanol (C2H5OH). Assuming CO2 is insoluble in H2O what would the pressure be of the CO2 inside the wine ...
Friday, November 16, 2007 at 1:27pm by mel

Chemistry
In the "Methode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is given below. C6H12O6(aq)--> 2 C2H5OH(aq) + 2 CO2(g) Fermentation of 746 mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total ...
Sunday, December 9, 2012 at 11:36pm by Alex

Chemistry
In the "Methode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is given below. C6H12O6(aq)--> 2 C2H5OH(aq) + 2 CO2(g) Fermentation of 746 mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total ...
Tuesday, December 11, 2012 at 9:27am by Alex

chemistry
In the "Methode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is given below. C6H12O6(aq)--> 2 C2H5OH(aq) + 2 CO2(g) Fermentation of 746 mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total ...
Tuesday, December 11, 2012 at 11:11pm by Alex

to dr bob..chemistry
bottle of wine contains 13.1% ethanol by volume. The density of ethanol (C2H5OH) is 0.789 g/cm3. Calculate the concentration of ethanol in wine in terms of mass percent and molality. mass percent _______% molality ______mol/kg Thanks Responses AP CHEMMMM - DrBob222, Saturday...
Sunday, November 30, 2008 at 11:28am by Lawrence

Chemistry: Dr. Bob, can you check my work?
In the "Methode Champenoise," grape juice is fermented in a wine bottle to produce sparkling wine. The reaction is given below. C6H12O6(aq) 2 C2H5OH(aq) + 2 CO2(g) Fermentation of 712 mL grape juice (density = 1.0 g/cm3) is allowed to take place in a bottle with a total volume...
Thursday, November 15, 2012 at 12:16am by Zachary

Chemistry
I found the moles of CO2 and I got 1.47. 85.4 L ethanol * .79 g/cm3 = 67.5g ethanol. 67.5/(12+12+5+16+1)= 1.47 moles ethanol. 1.47 moles C2H5OH *(2 moles C2H5OH/ 2 moles CO2) = 1.47 moles CO2. What do I use for the volume? do I use the volume of the bottle, the volume of the ...
Tuesday, November 13, 2012 at 7:56pm by Zachary

CHEMISTRY
ETHANOL (C2H5OH) HAS A DENSITY OF 0.80g/ml. IF A 10%(v/v) MIXTURE OF ETHANOL IN WATER WAS PREPARED HOW MANY GRAMS OF ETHANOL WOULD BE IN 100ML OF THE MIXTURE? (ASSUMING MIXED VOLUME IS THE SUM OF THE PARTIAL VOLUME)
Monday, April 25, 2011 at 10:40pm by PLEASE HELP!

Chemistry
14% (that's v/v) means 14 cc ethanol/100 cc wine so 750 cc wine x (14 cc ethanol/100 cc wine) = about 105 cc ethanol. 14 units x (10 cc ethanol/unit) = 140 cc ethanol 140 cc ethanol x (1 bottle/105 cc ethanol) = ? bottles
Saturday, February 8, 2014 at 10:36am by DrBob222

chemistry
Please help =) 59. Ethanol, C2H5OH, is responsible for the effects of intoxication felt after drinking alcoholic beverages. When ethanol burns in oxygen, carbon dioxide and water produced. (a) Write a balanced equation for the reaction. [[Think I did this right] Need help with...
Friday, October 10, 2008 at 11:19pm by shadow55

college chem
. Jack Daniels Tennessee whiskey is 40.00% ethanol by volume. However, % alcohol by mass is quite different from % by volume. The molality of ethanol in an aqueous solution that is 40.00 % ethanol by volume is 10.88 molal. A) Find the % ethanol by MASS, based on the molality. ...
Tuesday, March 9, 2010 at 11:11pm by josh

Chemistry: Dr. Bob, can you check my work?
I would use the volume of the bottle minus the volume of the ethanol. We're assuming all of the grape juice was glucose and all of it was converted to ethanol. Actually, since the grape juice was only 12% ethanol, I suppose the rest of it is water. The author of the problem ...
Thursday, November 15, 2012 at 12:16am by DrBob222

Chem
A bottle of win contains 12.5% ethanol by volume. The density of ethanol (C2H5OH) is .79 g/mL. Calculate the concentration of ethanol in wine as mass percent and molality. I calculated molality as 2.4 m/kg, but I'm stumped on the mass percent [although I'm hitting the right ...
Sunday, March 25, 2007 at 8:47pm by Jessica

chemistry
last check: (c) A wine cooler contains 4.5% ethanol by mass. Assuming that only the alcohol burns in oxygen, how many grams of wine cooler need to be burned to produce 3.12 L of CO2 (d = 1.80 g/L at 25C, 1 atm pressure) at the conditions given the density? 1 C2H5OH + 3 O2 = 2...
Sunday, October 12, 2008 at 12:08pm by starlight

chemistry
Calculate the molarity and mole fraction of a 2.35 m solution of acetone (CH3COCH3) dissolved in ethanol (C2H5OH). (Density of acetone = 0.788 g/cm3; density of ethanol = 0.789 g/cm3.) Assume that the final volume equals the sum of the volumes of acetone and ethanol.
Tuesday, May 4, 2010 at 2:00pm by bob

chemistry
The wine cooler problem is the same as the ethanol except that the wine cooler is not 100% ethanol. It is only 4.5%. Therefore, first find the mols CO2 you want to produce. Use PV = nRT. Convert mols CO2 to mols ethanol, then to grams ethanol. (I'll call the grams ethanol Y ...
Friday, October 10, 2008 at 11:19pm by DrBob222

Chemistry
Determine the molar concentration of ethanol (C2H6O) in a wine that is 14% ethanol by mass. The density of this wine is 0.93 g/cm^3.
Saturday, October 3, 2009 at 4:50pm by Anonymous

CHEMISTRY
An ethanol-water solution is prepared by dissolving 10.00 ml ethanol C2H5OH (density=0.789g/ml) in sufficient water to produce 100.00 ml of solution with a density of 0.982g/ml. What is the concentration of ethanol in this solution? Expressed as ml. a.)%volume b.)%mass c.)%m/v...
Wednesday, November 13, 2013 at 8:00am by ADRIAN

chemistry
What is the mass/vol % ethanol in an ethanol-water solution with density of 0.875 g/ml and containing 65.0% ethanol by volume? The density of pure ethanol is 0.789 g/ml.
Sunday, June 27, 2010 at 7:02pm by jimbo

Chemistry
C2H5OH + O2 -> C2H4O2 +H20 This reaction drastically changes the taste of wine, if 100.0 mL of wine initially contained 12.0 g of ethanol and after a period of time 4.00 g of acetic acid were detected, what percent of the ethanol had been converted?
Tuesday, June 7, 2011 at 7:39pm by Vinny

AP Chemistry
12.5% by volume means 12.5 mL ethanol/100 mL of solution. Don't we need the density of the wine in order to calculate the mass of the 100 mL? We can estimate if we assume ethanol and water volumes add (and I KNOW they do not). 12.5 mL ethanol in (12.5 mL ethanol+ 87.5 mL water...
Sunday, November 14, 2010 at 11:56pm by DrBob222

chemistry
60% (m/m)=60g of ethanol out of 100g in solution. 60g of ethanol*(1 mole/46.07g)= moles of ethanol Density=mass/volume Solving for volume, Volume=mass/density Total volume=100g total solution/0.8937g/ml Molarity=moles/volume in L Molarity of ethanol solution=moles of ethanol/...
Monday, July 29, 2013 at 1:35am by Devron

chemistry
A solution of ethanol, C2H5OH, is prepared by dissolving 25.0 mL of ethanol in enough water to give a total volume of 250.0 mL. What is the percent-by-volume concentration of ethanol?
Friday, May 10, 2013 at 10:44pm by Adrian

Chemistry
At 20 degrees C ethanol has a density of 0.789 g/ml and H2O has a density of 1.0 g/ml. What is the % by volume of ethanol of a solution made by adding 50g of ethanol with 50g of H2O? Tutor Answer: Use density = mass x volume to convert 50 g ethanol to volume and to convert 50....
Tuesday, November 29, 2011 at 9:24pm by Shelly

chemisty problem help
Carbon-12 contains 6 protons and 6 neutrons. The radius of the nucleus is approximately 70 pm. Calculate the volume of the nucleus and the volume of the atom. What percentage of the carbon atom's volume is occupied by the nucleus? Can someone tell me how to do this? Volume= 4/...
Thursday, February 8, 2007 at 9:42pm by Tagen

Chemistry
For ethanol, C2H5OH, which is mixed with gasoline to make the fuel gasohol, Hf = -277.63 kJ/mol. Based upon data in Table 6.2, and that the density of ethanol is 0.787 gcm-3, the number of kilojoules released by burning completely 2.40 gallons of ethanol is ? *Table 6.2 ...
Sunday, October 16, 2011 at 5:26pm by A

Chemistry #11
A solution of ethanol (C2H5OH) is prepared by dissolving 35.0 ml of ethanol in enough water to make 120.0 ml of solution. What is the molarity of the ethanol in this solution? 46.07 g= molar mass of ethanol .079 g/ml=density
Monday, October 14, 2013 at 11:15pm by Chelsea

chemistry
It would have helped if you wrote the equation. 2C2H5OH + 5O2 ==> 4CO2 + 6H2O 1.25 L H2O has a mass of 1.00 gram. 1.00 g H2O = ?? mols H2O. Convert mols H2O to mols C2H5OH using the coefficients in the balanced equation. Convert mols ethanol to grams ethanol. Using the ...
Friday, October 10, 2008 at 11:19pm by DrBob222

Chemistry
The density of an aqueous solution containing 10% of ethanol (C2H5OH) by mass is 0.984 g/ml. A) Calculate the molality of this solution. B) Calculate its molarity. C) What volume of the solution would contain 0.125 mol of ethanol.
Wednesday, March 17, 2010 at 11:40pm by Hilavidpreet

chemistry
Calculate the molarity and mole fraction of acetone in a 1.29 m solution of acetone (CH3COCH3) in ethanol (C2H5OH). (Density of acetone = 0.788 g/cm3; density of ethanol = 0.789 g/cm3.) Assume that the volumes of acetone and ethanol add.
Thursday, January 20, 2011 at 8:51pm by sarah

Chemistry
An aqueous solution of ethanol is 14.1M C2H5OH. The density of the solution is 0.853g/mL. What is molality of ethanol in the solution? What is mass % of ethanol in solution? I got the molality which is -21.7 ethanol, but I can't figure out how to get the mass % from the molality?
Monday, January 14, 2013 at 2:51pm by Robert

chem
calculate the number of grams of alcohol present in 1.70 L OF 75-Proof gin. The density of ethanol is 0.798 g/ml. Proof--> twice the % by volume of ethanol(C2H5OH) present.
Friday, January 28, 2011 at 4:24pm by help!

Chemistry
How much heat is required to convert 32.5 grams of ethanol at 28 C to the vapor phase at 78 C? Ethanol (C2H5OH) boils at 75 C. Its density is 0.789 g/mL. The enthalpy of vaporization is 38.56 kJ/mol. The specific heat of liquid ethanol is 2.3 J/g-K.
Thursday, February 11, 2010 at 9:24pm by Anonymous

Chemistry
A solution of ethanol (C2H5OH) in water is prepared by dissolving 76.9 mL of ethanol (density 0.79 g/cm^3) in enough water to make .250 L of solution. What is the molarity of ethanol in this solution?
Thursday, May 6, 2010 at 10:31am by Anonymous

apchem
A 15.0g sample of liquid ethanol, C2H5OH, absorbs 5.13x10^3 J of heat at its normal boiling point, 78.0C. The molar enthalpy of vaporization of ethanol is 39.3kJ/mol. (a) What volume of ethanol vapor is produced? The voume is measured at 78.0C and 1.00atm pressure. (b) What ...
Sunday, January 27, 2008 at 4:32pm by alk

Chemistry
A 15.0g sample of liquid ethanol, C2H5OH, absorbs 5.13x10^3 J of heat at its normal boiling point, 78.0C. The molar enthalpy of vaporization of ethanol is 39.3kJ/mol. (a) What volume of ethanol vapor is produced? The voume is measured at 78.0C and 1.00atm pressure. (b) What ...
Sunday, January 27, 2008 at 6:30pm by David

Chemistry
Calculate the volume (L) of the solute C4H8O and the volume (mL) of the solvent C2H5OH that should be combined to prepare 5.54 kg of a solution that is 0.608 m. Molar Mass (g/mol) C4H8O 72.12 C2H5OH 46.07 Density (kg/L): C4H8O 0.8892 C2H5OH 0.7893 Name/Formula: tetrahydrofuran...
Sunday, February 14, 2010 at 9:29pm by Jackie

chemistry
What is the percent by volume (% v/v) of a solution made by mixing 12 ml of ethanol (C2H5OH) with 48 ml of water? b) Assuming the density of ethanol is 0.789g/ml, what is the molarity of this solution?
Tuesday, March 19, 2013 at 4:52pm by ben

Science
You will require 0.873*0.768 = 0.6705 moles of ethanol. Its molar mass is 46 g/mol, so that is 30.84 g. Divide by the density of ethanol to get the ethanol volume, in ml.
Friday, March 8, 2013 at 12:51am by drwls

Chemistry
Use density = mass x volume to convert 50 g ethanol to volume and to convert 50.0 g H2O to volume. %ethanol v/v = (volume ethanol/total volume)*100 = ?
Monday, November 28, 2011 at 10:32pm by DrBob222

chem
drbob you helped me with this problem the other day but i have a question. -i changed 500mL of ethanol to grams then to mol. i was wondering if i then used 1000mL or 500mL of water to change to kg? The "proof" of an alcoholic beverage is twice the volume percent of ethanol, ...
Wednesday, February 13, 2008 at 4:33pm by alicia

Chemistry
Ethanol (C2H5OH) boils at a temperature of 78.3oC. What amount of energy, in joules, is necessary to heat to boiling and then completely vaporize a 28.6 g sample of ethanol initially at a temperature of 10.8oC. The specific heat of ethanol is approximately constant at 2.44 JK-...
Friday, October 7, 2011 at 9:27pm by John

chem
A solution of ethanol (C2H5OH) in water is prepared by dissolving 57.0 mL of ethanol (density = 0.79 g/cm3) in enough water to make 240.0 mL of solution. What is the molarity of the ethanol in this solution?
Saturday, November 3, 2007 at 11:31pm by mel

Chemistry
A solution of ethanol (C2H5OH) in water is prepared by dissolving 61.9 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?
Wednesday, October 27, 2010 at 11:58pm by Andrea

chemistry
A solution of ethanol (C2H5OH) in water is prepared by dissolving 87.4 mL of ethanol (density = 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution?
Monday, January 3, 2011 at 4:42pm by bob

chemistry
Problem#8: Metabolism of alcohol (ethanol, C2H5OH) by the body takes place according to the reaction: C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l) ΔHo = -1367 kJ Determine the number of food calories (Cal) supplied by the alcohol in a 12-oz (355-mL) bottle of Molson ...
Thursday, October 21, 2010 at 1:28pm by Sarah

chemistry
You have a solution that contains 340ml of water and 20ml of ethanol. Find the concentration of ethanol in this solution in each of the following units: (density of water is 1.00 g/ml, density of ethanol is 0.789g/ml)
Tuesday, February 18, 2014 at 5:02pm by Anonymous

Science
Assume you can heat water with perfect insulation (all the heat from combustion of ethanol is transferred to water). What is the volume of ethanol required to heat 100 mL of water by 10 degrees C? (You will need to look up density of ethanol, specific heat capacity or water, ...
Thursday, March 21, 2013 at 2:08am by Alexandra

Chemistry
Yes, you are right about density and no, I don't get those answers. For that density sentence I punched x instead of / button. density = mass/volume and volume = mass/density. 50 g ethanol has v = 50/0.789 or about 60 mL (but you need to do it more accurately). Water has ...
Tuesday, November 29, 2011 at 9:24pm by DrBob222

Chemistry -repost thank you in advance
I have a bottle of 95% ethanol purchased from the manufacturer. Normally, when it is not stated, does it mean 95% w/w ethanol? I need to prepare 100ml of 40% v/v ethanol solution from 95% ethanol. Please show me the calculation steps. Thanks.
Monday, September 20, 2010 at 10:33am by annie

science
Given that 6.20 x 10^23 ethanol molecules have a mass of 46.04g calculate the number of ethanol molecules in a film of ethanol that is 3.08 mm by 0.0015 mm. Assume the density of ethanol is 0.790 g/mL please helppp
Tuesday, August 28, 2012 at 3:06pm by anonymous

Chemistry
What is the mass/ vol% ethanol in an ethanol water solution with density of 0.875g/ml and containing 65% ethanol by volume? The density of pure ethanol is 0.789g/ml? My calculation 0.875g/ml x 1000ml x 0.65/ 46.06 = 12.34m 12.34/0.789g = 15.6g I am not sure answer. Pls help
Saturday, August 18, 2012 at 10:20pm by Fai

chem
The "proof" of an alcoholic beverage is twice the volume percent of ethanol, C2H5OH, in water. The density of ethanol is 0.789g/mL and that of water is 1.99g/mL. A bottle of 100-proof rum is left outside on a cold winter day. a) Will the rum freeze if the temperature drops to...
Tuesday, February 12, 2008 at 11:07am by alicia

chemistry
Ethanol (C2H5OH) melts at -114 C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (kJ) is needed to convert 25.0 g of solid ethanol at -135 C to liquid ethanol at -50 C?
Friday, February 3, 2012 at 1:24am by Anonymous

Chemistry
Mass of unknown solution=25.671 Mass ethanol =8.243 Assuming that prior experiments have shown the single-step extraction removes only 72.0 % of the ethanol, the mass of ethanol in your original unknown is 11.45 Mass percent ethanol =44.6 % Given a density of 0.789 g/mL, what ...
Sunday, January 29, 2012 at 10:18pm by Forrest

science
ethanol, C2H5OH, is responsible for the effts of intoxication felt after drinking alcoholic beverages. When ethanol burns in oxygen, carbon dioxide and water are produced. IF you have 256g of ethanol and 100 grams O2, calculate the amount product produced. You need to write ...
Sunday, February 6, 2011 at 4:43pm by liz

Chemistry
At 20 degrees C ethanol has a density of 0.789 g/ml and H2O has a density of 1.0 g/ml. What is the % by volume of ethanol of a solution made by adding 50g of ethanol with 50g of H2O?
Monday, November 28, 2011 at 10:32pm by Shelly

chemistry
Calculate the mass ( g ) of the solute ethanol and the mass ( kg ) of the solvent CHCl3 that should be combined to prepare 9900 g of a solution that is 14.5 m ethanol. extra given info from problem: molar mass (g/mol): C2H5OH 46.07 CHCl3 119.38 density (kg/L): C2H5OH 0.7893 ...
Thursday, February 25, 2010 at 8:03pm by Diem

chemistry
What volume of 0.210 ethanol solution contains .44 mol ethanol?
Thursday, April 1, 2010 at 6:56pm by Anonymous

chemistry
What volume of 0.210 WHAT ethanol solution contains .44 mol ethanol?
Thursday, April 1, 2010 at 6:56pm by DrBob222

AP CHEMMMM
I suppose you are to assume the density of the ine to be 1.00. I looked up the density of wine on the Internet and found that it varies between about 0.990 to 1.01 so 100 mL would have a mass of 99 to 101 which isn't that far from 100. So 13.1% v/v means 13.1 mL ethanol/100 mL...
Saturday, November 29, 2008 at 10:22pm by DrBob222

chemistry
Calculate the volume ( mL ) of the solute C2H5OH and the mass ( g ) of the solvent diethyl ether that should be mixed to produce 3.46 kg of a solution that is 1.31 m C2H5OH. volume ( mL ) of the C2H5OH mass ( g ) of the (C2H5)2O Molar Mass (g/mol) C2H5OH 46.07 (C2H5)2O 74.12 ...
Thursday, June 3, 2010 at 10:48pm by Judy

Chemistry
Ethanol (C2H5OH) boils at a temperature of 78.3oC. What amount of energy, in joules, is necessary to heat to boiling and then completely vaporize a 22.8 g sample of ethanol initially at a temperature of 16.5oC. The specific heat of ethanol is approximately constant at 2.44 JK-...
Thursday, October 6, 2011 at 12:40pm by tanner

Chemistry
Ethanol (C2H5OH) boils at a temperature of 78.3oC. What amount of energy, in joules, is necessary to heat to boiling and then completely vaporize a 13.1 g sample of ethanol initially at a temperature of 11.1oC. The specific heat of ethanol is approximately constant at 2.44 JK-...
Thursday, October 6, 2011 at 2:53pm by Carrie

Chemistry
Gasohol contains ethanol (C2H4OH)(l), which when burned reacts with oxygen to produce CO2(g) and H2O(g). How much heat is released when 12.5g of ethanol burns? C2H5OH(l) + 3 O2(g) --> 2 CO2(g) + 3H2O(l) Delta H = -1368kJ
Wednesday, May 19, 2010 at 8:42pm by Keith

chem
A 4.1 L sealed bottle containing 0.25 g of liquid ethanol, C2H6O, is placed in a refrigerator and reaches equilibrium with its vapor at -11C. The vapor pressure of ethanol is 10 torr at -2.3C and 40 torr at 19C. (a) What mass of ethanol is present in the vapor?
Sunday, November 14, 2010 at 9:23pm by Anonymous

Chemistry
Ethanol, C2H5OH, is mixed with gasoline and sold as gasohol. Use the following to calculate the grams of ethanol needed to provide 367 kJ of heat. C2H5OH(l) + 3 O2(g) 2 CO2(g) + 3 H2O(g) H = −1235 kJ
Monday, November 21, 2011 at 5:29pm by Samantha

college chem
Ethanol (C2H5OH) boils at a temperature of 78.3oC. What amount of energy, in joules, is necessary to heat to boiling and then completely vaporize a 20.0 g sample of ethanol initially at a temperature of 13.6oC. The specific heat of ethanol is approximately constant at 2.44 JK-...
Tuesday, October 4, 2011 at 3:56pm by john

CHEMISTRY STOICHIOMETRY!!!!!!!!
AN an antacid tablet contains 0.1g of magnesium hydrocarbonate, what nass of stomach acid, HCL, will it neutralise? Wine is made by the fermentation of the sugar in grapes. Surose-> Ethanol+Carbondioxide. Whta massof ethanol can be obtained from 6.00kg of sucrose?
Saturday, November 10, 2007 at 7:44am by akan

Chemistry
Gasohol contains ethanol (C2H4OH)(l), which when burned reacts with oxygen to produce CO2(g) and H2O(g). How much heat is released when 12.5g of ethanol burns? C2H5OH(l) + 3 O2(g) --> 2 CO2(g) + 3H2O(l) Delta H = -1368kJ How do I solve this problem?
Wednesday, May 19, 2010 at 10:44pm by Kieth

Chemistry
Calculate the mass of ethanol (m) used from the volume and the density. Calculate the RMM for ethanol Then use m/RMM to calculate the number of moles (M) of ethanol. I presume the final volume is 0.250 L rather than 250 L. The molarity is then M/0.250 L
Thursday, May 6, 2010 at 10:31am by Dr Russ

Chemistry
Use density to convert 125.0 mL ethanol to grams. mass = volume x density q = mass ethanol x deltaHvap = ??
Wednesday, January 19, 2011 at 11:43am by DrBob222

Chemistry
Hydrogren, a possible future fuel, can also be obtained from other compounds such as ethanol. Ethanol can be made from the fermentation of crops, such as corn. How much hydrogen in grams can be obtained from 1.0 kg of ethanol (C2H5OH)?
Tuesday, April 1, 2008 at 4:19pm by Kate

Water solubility chemistry
What solvent that would dissolve Ethanol in water? You mean selectively dissolve the ethanol out of the water? Ethanol is soluble in water, at least last night when I had wine, it was dissolved. I dont know of anything that selectively absorbes ethanol when dissolved in water.
Sunday, March 25, 2007 at 12:03pm by Hasina

Chemistry
A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb calorimeter. The temperature of the calorimeter rose from 25.00C to 33.73C. If the heat capacity of the calorimeter and contents was 9.63 kJ/C, what is the value of q for burning 1.28 ...
Tuesday, June 7, 2011 at 8:26am by Lance

chemistry
Ethanol has a density of 0.780 g/mL. What volume would 500. grams of ethanol occupy. Answer with correct number of sig figs
Tuesday, January 31, 2012 at 7:05pm by kr

chem
mass = volume x density. Use this to calculate the mass of ethanol. mols ethanol = grams/molar mass. M = mols/L = mols ethanol/0.240 L = ??
Saturday, November 3, 2007 at 11:31pm by DrBob222

Chemistry
The heat energy of ethanol is 29800J/g. A 355g can of beer contains 3.70% ethanol by mass. How many ethanol calories are in a can of beer?
Wednesday, March 11, 2009 at 1:19pm by Kayla

economics
Assume that a bottle of wine sells for $10. The government decides to put a $1 per bottle tax on wine. What will be the new price that consumers must pay for a bottle of wine?
Sunday, February 28, 2010 at 10:22pm by Anonymous

chemistry
An aqueous solution of ethanol is 3.05 M in ethanol, CH3CH2OH. Calculate the mole fraction of ethanol if the density of the solution is 0.964 g mL-1.
Monday, November 12, 2007 at 10:43am by mark

Chemistry
What mass of water must be used to dissolve 20.0 grams of ethanol, C2H5OH, to prepare a 0.0500 molal solution of ethanol?
Sunday, February 10, 2013 at 3:45am by Marcus

chemistry
ethanol(C2H5OH)and gasoline(assumed to be octane,C8H18) are both used as automobile fuel.if gasoline is selling for $2.20/gal,what would the price of ethanol have to be in order to provide the same amount of heat per dollar?The density and ΔHf of octane are 0.7025g/ml and...
Wednesday, November 2, 2011 at 10:55pm by asembi

Chemistry
It would have helped to give the data below. Here is how you do the problem. I assume there is a density. Use the density to calculate the mass. mass -= volume x density. Then for heat used there are two formula to use. Within a phase you use mass x specific heat x (Tfinal-...
Thursday, March 8, 2012 at 6:40pm by DrBob222

chemistry
1.) How much ethanol, C2H5OH, in liters (d=0.789g/ml) must be dissolved in water to produce 190.5 of 1.65 M C2H5OH? (Molarity problem.) 190.5 WHAT for crying out loud?barrels, freight cars, lakes, I will assume you meant mL. If not that, adjust values below to what you should ...
Friday, February 12, 2010 at 8:22pm by DrBob222

chemistry
you have 23- grams sample of ethanol with a density of 0.7893g/ml what volume of ethanol do you have?
Monday, September 27, 2010 at 8:08am by trice

chemistry
You have a 22 g sample of ethanol with a density of 0.7893 g/mL. What volume of ethanol do you have?
Tuesday, September 14, 2010 at 7:42pm by Anonymous

chemistry
You have a 22 g sample of ethanol with a density of 0.7893 g/mL. What volume of ethanol do you have?
Monday, August 15, 2011 at 7:57pm by patricia

chemistry
2.35 m. Take enough solution to have 2.35 moles. That mans you have 1 kg solvent (ethanol). volume ethanol = m/d = 1000g/0.789 = ??. 2.35 mol acetone x molar mass acetone = grams acetone and mass/density = volume. Add volume acetone to volume ethanol to find total volume. Then...
Tuesday, May 4, 2010 at 2:00pm by DrBob222

chemistry
Calculate enthalpy change of reaction for the combustion of gaseous ethanol. C2H5OH + 3O2 >> CO2 + 3H2O. Using standard molar enthalpies of formation. C2H5OH -235.3 ( it's negative sign) CO2 -393.5 H2O -241.8 (1) Calculate the enthalpy change of reaction per mole of ...
Tuesday, April 20, 2010 at 10:00am by Alex

chemistry
use a combustion reaction of liquid ethanol( C2H5OH) an air as a source of work, assuming T=25 celcius, air pressure is 1 atm, and all products are gases with partial pressure of 10 atm each. How high can one lift a 1000 kg weight by burning 100 g of ethanol. note oxygen is 21...
Sunday, November 7, 2010 at 7:47pm by Whitney

chemistry
C2H5OH + 3O2 --> 2CO2 + 3H2O How many grams of O2 are consumed when 5.86 ml of Ethanol burns completely (the density of C2H5OH is 0.789 g/ml)?
Thursday, February 16, 2012 at 8:19pm by Delta

chemistry
use density to convert volume ethanol and volume H2O to mass in grams. Then [mass ethanol x specific heat ethanol x (Tfinal-Tinitial)] + [mass H2O x specific heat H2O x (Tfinal-Tinitial)] = 0. Substitute and solve for Tfinal. You must look up specific heat ethanol and H2O.
Tuesday, October 15, 2013 at 1:14am by DrBob222

chemistry
What is the maximum amount of ethanol (in grams) that can be produced when 1.0 kg of ethylene (C2H4) and 0.014 kg of steam are placed into the reaction vessel? Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very high pressure. C2H4...
Tuesday, November 1, 2011 at 10:29am by Amanda

Chemistry
Ethanol (C2H5OH) is synthesized for industrial use by the following reaction, carried out at very high pressure. C2H4(g) + H2O(g) C2H5OH(l) What is the maximum amount of ethanol (in grams) that can be produced when 1.0 kg of ethylene (C2H4) and 0.014 kg of steam are placed ...
Tuesday, November 1, 2011 at 10:33am by Jack

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