What will have the lowest percent composition in the dehydration of 2-butanol and why?
Q. In the dehydration of 2-bromobutane, trans-2-butene has the largest percent composition and cis-2-butene has the lowest percent composition. Why does 1-butene have the lowest percent composition in dehydration of 2-butanol? Or are these results just wrong?
Asked by Michelle - Thu Nov 12 13:14:34 2009 - - 1 Answers - 0 Comments
Q. In the dehydration of 2-bromobutane, trans-2-butene has the largest percent composition and cis-2-butene has the lowest percent composition. Why does 1-butene have the lowest percent composition in dehydration of 2-butanol? Or are these results just wrong?
Asked by Michelle - Thu Nov 12 13:14:34 2009 - - 1 Answers - 0 Comments
What is the mass percent composition of sodium carbonate using stoichiometry?
Q. A 9.052g mixture of sodium carbonate and sodium chloride contains 3.7130g of sodium. What is the mass percent composition of the mixture? The answer to it is 41.58% sodium carbonate. What I don't know is how to get to the answer. Please help!
Asked by anonymous - Tue Sep 8 12:33:25 2009 - - 1 Answers - 0 Comments
A. let x = mass Na2CO3 let y = mass NaCl x + y = 9.052 moles Na = 3.7130 g/ 22.9898 g/mol=0.1615 2x/ 121.9866 + y / 58.4428 = 0.1615 y= 9.052 - x 2x / 121.9866 + 9.052 - x/ 58.4428= 0.1615 solve for x = mass Na2CO3 % = mass Na2CO3 x 100/ 9.052
Answered by Dr.A - Tue Sep 8 13:15:31 2009
Q. A 9.052g mixture of sodium carbonate and sodium chloride contains 3.7130g of sodium. What is the mass percent composition of the mixture? The answer to it is 41.58% sodium carbonate. What I don't know is how to get to the answer. Please help!
Asked by anonymous - Tue Sep 8 12:33:25 2009 - - 1 Answers - 0 Comments
A. let x = mass Na2CO3 let y = mass NaCl x + y = 9.052 moles Na = 3.7130 g/ 22.9898 g/mol=0.1615 2x/ 121.9866 + y / 58.4428 = 0.1615 y= 9.052 - x 2x / 121.9866 + 9.052 - x/ 58.4428= 0.1615 solve for x = mass Na2CO3 % = mass Na2CO3 x 100/ 9.052
Answered by Dr.A - Tue Sep 8 13:15:31 2009
What is the percent composition of a mixture?
Q. Question:What is the percent composition of sodium chloride, sand, and iron mixture? You must retain all of the reactant? I have to develop a procedure to separate all the components. How would i do that? I know that to find the iron, i can use a magnet, but how do i separate the salt from the sand?
Asked by carlos - Mon Jun 8 18:29:41 2009 - - 1 Answers - 0 Comments
A. If you put them in water and heat it, then the sodium chloride will dissolve and the sand will not, so you can filter the sand. The salt will probably come back out when you cool the water and then put it on ice... but I might be wrong and it might not come out. Use as little water as possible?
Answered by unknown - Mon Jun 8 18:37:55 2009
Q. Question:What is the percent composition of sodium chloride, sand, and iron mixture? You must retain all of the reactant? I have to develop a procedure to separate all the components. How would i do that? I know that to find the iron, i can use a magnet, but how do i separate the salt from the sand?
Asked by carlos - Mon Jun 8 18:29:41 2009 - - 1 Answers - 0 Comments
A. If you put them in water and heat it, then the sodium chloride will dissolve and the sand will not, so you can filter the sand. The salt will probably come back out when you cool the water and then put it on ice... but I might be wrong and it might not come out. Use as little water as possible?
Answered by unknown - Mon Jun 8 18:37:55 2009
How to solve this chemistry problem about percent composition?
Q. An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. Determine the percent composition of the substance.
Asked by Tony - Thu May 14 00:10:05 2009 - - 1 Answers - 0 Comments
A. This is a bit tedious, but you just have to work through it. Volume of one mole of gas at STP: 22.4 litres. Moles of CO2 produced: 83.16 / 22400 = 0.00371 One mole of C per mole of CO2 : 0.00371 12 grams per mole of C : 0.04455 grams or 44.55mg of C. Moles of H2O produced: 73.30 / 22400 = 0.00327 Two moles of H per mole of H2O : 0.00654 One gram per mole of H : 0.00654 grams or 6.54mg of H. 44.55mg of C + 6.54mg of H + 16.44 mg of Cl = 67.53 Subtract that from 100.00mg, leaves 32.47mg of N. Because the sample is 100mg, those are also the percentage compositions by weight. Just one awkward observation: how do we get 73.30 mL of H2O vapor at STP ? At STP, the water would be liquid, on the point of freezing..
Answered by WhatGoes Around Comes Around - Sun May 17 21:29:27 2009
Q. An herbicide is found to contain only C, H, N, and Cl. The complete combustion of a 100.0-mg sample of the herbicide in excess oxygen produces 83.16 mL of CO2 and 73.30 mL of H2O vapor at STP. A separate analysis shows that the sample also contains 16.44 mg of Cl. Determine the percent composition of the substance.
Asked by Tony - Thu May 14 00:10:05 2009 - - 1 Answers - 0 Comments
A. This is a bit tedious, but you just have to work through it. Volume of one mole of gas at STP: 22.4 litres. Moles of CO2 produced: 83.16 / 22400 = 0.00371 One mole of C per mole of CO2 : 0.00371 12 grams per mole of C : 0.04455 grams or 44.55mg of C. Moles of H2O produced: 73.30 / 22400 = 0.00327 Two moles of H per mole of H2O : 0.00654 One gram per mole of H : 0.00654 grams or 6.54mg of H. 44.55mg of C + 6.54mg of H + 16.44 mg of Cl = 67.53 Subtract that from 100.00mg, leaves 32.47mg of N. Because the sample is 100mg, those are also the percentage compositions by weight. Just one awkward observation: how do we get 73.30 mL of H2O vapor at STP ? At STP, the water would be liquid, on the point of freezing..
Answered by WhatGoes Around Comes Around - Sun May 17 21:29:27 2009
How do you find the percent composition of casein?
Q. How do you find the percent composition of casein when it's isolated from milk.
Asked by amanda f - Mon May 28 19:00:49 2007 - - 1 Answers - 0 Comments
A. Do a gravimetric analysis.
Answered by ag_iitkgp - Tue May 29 13:31:56 2007
Q. How do you find the percent composition of casein when it's isolated from milk.
Asked by amanda f - Mon May 28 19:00:49 2007 - - 1 Answers - 0 Comments
A. Do a gravimetric analysis.
Answered by ag_iitkgp - Tue May 29 13:31:56 2007
What is the percent composition by mass of sodium chloride in an aqueous solution of sodium chloride that has?
Q. What is the percent composition by mass of sodium chloride in an aqueous solution of sodium chloride that has a molar concentration of 2.23 M and density of 1.01 g/mL?
Asked by jack - Tue Mar 4 17:53:55 2008 - - 1 Answers - 0 Comments
A. Let us take 1l of solution. It will weigh 1*density or 1.02kg Now we need to work out the level of NaCl present. The number of moles = molarity *vol = 2.23* 1 =2.23 moles NaCl in 1 l of solution The mass of NaCl = moles * atomic weight = 2.23 * (23.0 + 35.5) = 130 g NaCl in 1 l of soln = 0.130kg Therefore the % NaCl = 0.130/ 1.01 = 12.9%
Answered by ktrna69 - Tue Mar 4 18:04:12 2008
Q. What is the percent composition by mass of sodium chloride in an aqueous solution of sodium chloride that has a molar concentration of 2.23 M and density of 1.01 g/mL?
Asked by jack - Tue Mar 4 17:53:55 2008 - - 1 Answers - 0 Comments
A. Let us take 1l of solution. It will weigh 1*density or 1.02kg Now we need to work out the level of NaCl present. The number of moles = molarity *vol = 2.23* 1 =2.23 moles NaCl in 1 l of solution The mass of NaCl = moles * atomic weight = 2.23 * (23.0 + 35.5) = 130 g NaCl in 1 l of soln = 0.130kg Therefore the % NaCl = 0.130/ 1.01 = 12.9%
Answered by ktrna69 - Tue Mar 4 18:04:12 2008
How do i calculate percent composition when only given the average atomic mass?
Q. the atomic mass of lithium 6 is 6.0151 amu and the atomic mass of lithium 7 is 7.0160. if the average mass of a sample of lithium in 6.941 ammu, what is the percent composition of each element?
Asked by tina r - Fri Aug 28 18:24:19 2009 - - 2 Answers - 0 Comments
A. You know lithium is either 6Li or 7Li, so the fractions add up to unity. So let's say that x of the Li is 7; and 1-x is 6. fraction 6*mass of 6 + fraction 7 * mass of 7 = average mass (1-x)*6.0151 + x*7.0160 = 6.941 6.0151 - 6.0151x +7.0160 x = 6.941 x(7.0160-6.0151) = 6.941-6.0151 1.0009x = 0.9259 x = 0.9251; 1-x = 0.0749 92.51% 7; 7.49% 6
Answered by unknown - Fri Aug 28 18:32:53 2009
Q. the atomic mass of lithium 6 is 6.0151 amu and the atomic mass of lithium 7 is 7.0160. if the average mass of a sample of lithium in 6.941 ammu, what is the percent composition of each element?
Asked by tina r - Fri Aug 28 18:24:19 2009 - - 2 Answers - 0 Comments
A. You know lithium is either 6Li or 7Li, so the fractions add up to unity. So let's say that x of the Li is 7; and 1-x is 6. fraction 6*mass of 6 + fraction 7 * mass of 7 = average mass (1-x)*6.0151 + x*7.0160 = 6.941 6.0151 - 6.0151x +7.0160 x = 6.941 x(7.0160-6.0151) = 6.941-6.0151 1.0009x = 0.9259 x = 0.9251; 1-x = 0.0749 92.51% 7; 7.49% 6
Answered by unknown - Fri Aug 28 18:32:53 2009
How do I find the percent of composition of these numbers?
Q. I'm trying to find the percent composition (mass) of these two numbers from a science experiment: 2.40 and 1.0 g/ml
Asked by Brian - Mon Aug 20 12:39:00 2007 - - 1 Answers - 0 Comments
A. The term 'percent of composition' is not a term which can sensibly be applied to the numbers themselves. I guess what you want is the percentage composition of a mixture containing 2.40 g/ml of A and 1.0 g/ml of B. If that is so, then the percentage of A is: 2.4 * 100 / (2.4 + 1.0) = 240 / 3.4 = 70.59% and the percentage of B is: 1.0 * 100 / (2.4 + 1.0) which you will find is equal to: 100 - 70.59 = 29.41%
Answered by unknown - Mon Aug 20 13:53:27 2007
Q. I'm trying to find the percent composition (mass) of these two numbers from a science experiment: 2.40 and 1.0 g/ml
Asked by Brian - Mon Aug 20 12:39:00 2007 - - 1 Answers - 0 Comments
A. The term 'percent of composition' is not a term which can sensibly be applied to the numbers themselves. I guess what you want is the percentage composition of a mixture containing 2.40 g/ml of A and 1.0 g/ml of B. If that is so, then the percentage of A is: 2.4 * 100 / (2.4 + 1.0) = 240 / 3.4 = 70.59% and the percentage of B is: 1.0 * 100 / (2.4 + 1.0) which you will find is equal to: 100 - 70.59 = 29.41%
Answered by unknown - Mon Aug 20 13:53:27 2007
How to do percent composition using dimensional analysis?
Q. I have a test tomorrow and i have to use dimensional analysis to find the percent composition here's a problem in my quiz if someone could help me thanks Calculate the percent of composition of a. carbon and hydrogen in lithum acetate(LiC2H3O2) b. Tin in Tin(IV)oxide
Asked by kobivr - Sun Mar 9 22:16:22 2008 - - 1 Answers - 0 Comments
A. Recall that any percent is sample / total. FInd the atomic mass of what you are looking for and for the sample: C = 12 g/mol LiC2H3O3 = 82 g/mol 12 g/mol / 82 g/mol = 0.146 x 100 = 14.6% C
Answered by drbillmacmo - Sun Mar 9 22:21:46 2008
Q. I have a test tomorrow and i have to use dimensional analysis to find the percent composition here's a problem in my quiz if someone could help me thanks Calculate the percent of composition of a. carbon and hydrogen in lithum acetate(LiC2H3O2) b. Tin in Tin(IV)oxide
Asked by kobivr - Sun Mar 9 22:16:22 2008 - - 1 Answers - 0 Comments
A. Recall that any percent is sample / total. FInd the atomic mass of what you are looking for and for the sample: C = 12 g/mol LiC2H3O3 = 82 g/mol 12 g/mol / 82 g/mol = 0.146 x 100 = 14.6% C
Answered by drbillmacmo - Sun Mar 9 22:21:46 2008
What is the percent composition by mass?
Q. Calculate the percent composition and determine the molecular formula and the empirical formula for the hydrogen-oxygen compound that results when 2.83 g of hydrogen is reacted with enough oxygen to produce 25.5 g of product. The molar mass of the product is 18.0 g. What is the percent composition by mass? percent oxygen: % percent hydrogen: % The molecular formula of the compound? q41
Asked by whocares! - Fri Apr 4 14:53:25 2008 - - 1 Answers - 0 Comments
A. 2.83 g of hydrogen @ 1 g / mol =2.83 mol H 25.5 g of product - 2.83 g H = 22.67 g oxygen 22.67 g oxygen @ 16 g/ mol = 1.42 mol oxygen --- 2.83 mol H / 0.283 = 1 part H 1.42 mol oxygen / 0.283 = 0.5 parts Oxygen double both = empirical formula = H2O --- @ 18 g/mol, molecular formula = also H2O --- % oxygen = 22.67 g oxy / 25.5 g total = 88.9 % oxygen % Hydrogen = 2.83 g / 25.5 g total = 11.1 % hydrogen
Answered by Steve O - Fri Apr 4 18:19:21 2008
Q. Calculate the percent composition and determine the molecular formula and the empirical formula for the hydrogen-oxygen compound that results when 2.83 g of hydrogen is reacted with enough oxygen to produce 25.5 g of product. The molar mass of the product is 18.0 g. What is the percent composition by mass? percent oxygen: % percent hydrogen: % The molecular formula of the compound? q41
Asked by whocares! - Fri Apr 4 14:53:25 2008 - - 1 Answers - 0 Comments
A. 2.83 g of hydrogen @ 1 g / mol =2.83 mol H 25.5 g of product - 2.83 g H = 22.67 g oxygen 22.67 g oxygen @ 16 g/ mol = 1.42 mol oxygen --- 2.83 mol H / 0.283 = 1 part H 1.42 mol oxygen / 0.283 = 0.5 parts Oxygen double both = empirical formula = H2O --- @ 18 g/mol, molecular formula = also H2O --- % oxygen = 22.67 g oxy / 25.5 g total = 88.9 % oxygen % Hydrogen = 2.83 g / 25.5 g total = 11.1 % hydrogen
Answered by Steve O - Fri Apr 4 18:19:21 2008
How do I do these percent composition problems?
Q. Calculate the percent composition of each of the following compounds: (A) C14H18N2O5 (B) SiC (C) C9H8O4
Asked by Alvy - Sun Sep 21 15:43:47 2008 - - 1 Answers - 0 Comments
A. A) There are 14 moles from C, 18 moles from H, 2 moles from N and 5 moles from O. In all= 39 moles 39--->100% 18---> x x = 18/39 x 100 = 0.46 x 100 = 46% Carbon you must do the same with the rest
Answered by Tom ate - Sun Sep 21 15:53:28 2008
Q. Calculate the percent composition of each of the following compounds: (A) C14H18N2O5 (B) SiC (C) C9H8O4
Asked by Alvy - Sun Sep 21 15:43:47 2008 - - 1 Answers - 0 Comments
A. A) There are 14 moles from C, 18 moles from H, 2 moles from N and 5 moles from O. In all= 39 moles 39--->100% 18---> x x = 18/39 x 100 = 0.46 x 100 = 46% Carbon you must do the same with the rest
Answered by Tom ate - Sun Sep 21 15:53:28 2008
How do I solve this percent composition?
Q. Find the percent composition of a compound that contains 1.94g of carbon, 0.48g of hydrogen, and 2.58g of sulfur in a 5.00g sample of the compound. Thanks
Asked by totiredtotalk - Sun Mar 1 18:07:15 2009 - - 1 Answers - 0 Comments
Q. Find the percent composition of a compound that contains 1.94g of carbon, 0.48g of hydrogen, and 2.58g of sulfur in a 5.00g sample of the compound. Thanks
Asked by totiredtotalk - Sun Mar 1 18:07:15 2009 - - 1 Answers - 0 Comments
What is the empirical formula of the compound with a mass percent composition of 70.0% Fe and 30.0% O?
Q. What is the empirical formula of the compound with a mass percent composition of 70.0% Fe and 30.0% O? . (Keep the elements in the order given.)
Asked by College Inof Needed - Thu Nov 6 00:09:15 2008 - - 2 Answers - 0 Comments
A. FeO2, if i did the math right. you take the percents and act like theyre grams and then convert to moles, so 70% Fe becomes 1.25 moles and 30% O comes out to about 1.8 moles. then you divide both by the smallest # and you get how many molecules of each, and you have to round up b.c when you divide 1.8 by 1.26 you get 1.5 or something like that, and you round up to 2. :] hope that helped, i kinda suck at teaching and explaining but im pretty good at chem
Answered by Kathleen S - Thu Nov 6 00:18:23 2008
Q. What is the empirical formula of the compound with a mass percent composition of 70.0% Fe and 30.0% O? . (Keep the elements in the order given.)
Asked by College Inof Needed - Thu Nov 6 00:09:15 2008 - - 2 Answers - 0 Comments
A. FeO2, if i did the math right. you take the percents and act like theyre grams and then convert to moles, so 70% Fe becomes 1.25 moles and 30% O comes out to about 1.8 moles. then you divide both by the smallest # and you get how many molecules of each, and you have to round up b.c when you divide 1.8 by 1.26 you get 1.5 or something like that, and you round up to 2. :] hope that helped, i kinda suck at teaching and explaining but im pretty good at chem
Answered by Kathleen S - Thu Nov 6 00:18:23 2008
what is the percent composition of phosphorous pentachloride?
Q. what is the percent composition of phosphorous pentachloride?
Asked by checojoel - Tue Apr 1 15:44:22 2008 - - 1 Answers - 0 Comments
A. Ok, the formula is P(Cl)5. Now take a periodic table, calculate the molecular weight of this compound. Then, take the atomic weight of P and divide by the molecular mass and multiply by 100, that is your percent composition for phosphorous. Do the same with Cl, don't forget to multiply by 5! The two numbers have to add up to 100.
Answered by sunshinegirl - Tue Apr 1 16:04:38 2008
Q. what is the percent composition of phosphorous pentachloride?
Asked by checojoel - Tue Apr 1 15:44:22 2008 - - 1 Answers - 0 Comments
A. Ok, the formula is P(Cl)5. Now take a periodic table, calculate the molecular weight of this compound. Then, take the atomic weight of P and divide by the molecular mass and multiply by 100, that is your percent composition for phosphorous. Do the same with Cl, don't forget to multiply by 5! The two numbers have to add up to 100.
Answered by sunshinegirl - Tue Apr 1 16:04:38 2008
Need to find the molecular formula of a compound with the percent composition and molar mass given.?
Q. Given: The percent composition of caffeine is 49.5% C, 5.20% H, 16.5% O, 28.9% N. What is the molar formula of caffeine if its molar mass is 194.1 g/mol? Thank you so much, im so confused on this one and if anyone knows please answer! peace
Asked by freedom.peace_love - Sat Mar 29 11:34:34 2008 - - 1 Answers - 0 Comments
A. how to find the molecular formula: 1) Determine the empirical formula of substance 2) Find the mass of the empirical formula. 3) Divide the mass of the substance by the empirical mass of substance to get a whole number. 4) Multiply the empirical formula by the whole number to get the molecular formula. Okay, so : 1) use the % composition to determine the empirical formula. Since it is a percentage, assume you have 100 g of caffeine in total. #moles = mass of element in 100g/atomic mass so, n (#of moles) for C = 49.5g/12.01 = 4.12 mol n for H = 5.20g / 1.01 = 5.15 mol n for O = 16.5g / 16.00 = 1.03 mol n for N = 28.9g / 14.00 = 2.06 mol With these moles determine the whole number ratio by dividing the molar amounts by the lowest molar… [cont.]
Answered by Gavindecaribou - Sat Mar 29 15:17:25 2008
Q. Given: The percent composition of caffeine is 49.5% C, 5.20% H, 16.5% O, 28.9% N. What is the molar formula of caffeine if its molar mass is 194.1 g/mol? Thank you so much, im so confused on this one and if anyone knows please answer! peace
Asked by freedom.peace_love - Sat Mar 29 11:34:34 2008 - - 1 Answers - 0 Comments
A. how to find the molecular formula: 1) Determine the empirical formula of substance 2) Find the mass of the empirical formula. 3) Divide the mass of the substance by the empirical mass of substance to get a whole number. 4) Multiply the empirical formula by the whole number to get the molecular formula. Okay, so : 1) use the % composition to determine the empirical formula. Since it is a percentage, assume you have 100 g of caffeine in total. #moles = mass of element in 100g/atomic mass so, n (#of moles) for C = 49.5g/12.01 = 4.12 mol n for H = 5.20g / 1.01 = 5.15 mol n for O = 16.5g / 16.00 = 1.03 mol n for N = 28.9g / 14.00 = 2.06 mol With these moles determine the whole number ratio by dividing the molar amounts by the lowest molar… [cont.]
Answered by Gavindecaribou - Sat Mar 29 15:17:25 2008
How do i find the molecular formula of a compound when given the percent composition of each element?
Q. A compound with a molar mass of 100. g/mol has an elemental composition of 24.% C, 3.% H, 16.% O, and 57.% E. How do i find the molecular formula of this compound?
Asked by kcc - Tue Feb 13 20:11:13 2007 - - 2 Answers - 0 Comments
A. what is E? There are 2 parts carbon, 3 parts hydrogen, 1 part oxygen.
Answered by yungr01 - Tue Feb 13 20:15:07 2007
Q. A compound with a molar mass of 100. g/mol has an elemental composition of 24.% C, 3.% H, 16.% O, and 57.% E. How do i find the molecular formula of this compound?
Asked by kcc - Tue Feb 13 20:11:13 2007 - - 2 Answers - 0 Comments
A. what is E? There are 2 parts carbon, 3 parts hydrogen, 1 part oxygen.
Answered by yungr01 - Tue Feb 13 20:15:07 2007
What is the percent composition of oxygen in 15 grams of ammonium hydroxide?
Q. I know how to do this really. I'm not really asking you for the answer. I just wanna know how to do it right. But the 15 grams thing is throwing me off. Am I dividing 15 grams by the oxygen molar mass or am I dividing the whole molar mass by oxygen molar mass? I'm really confused, please help!!
Asked by suzy - Fri Feb 29 20:03:44 2008 - - 2 Answers - 0 Comments
A. I'm glad you said you know how to do this. As far as doing it right, you already did. The 15 grams extra information. A teacher would probably not give you any partial credit if you used the 15 grams in a calculation. Good Job!
Answered by Derrick - Fri Feb 29 20:28:02 2008
Q. I know how to do this really. I'm not really asking you for the answer. I just wanna know how to do it right. But the 15 grams thing is throwing me off. Am I dividing 15 grams by the oxygen molar mass or am I dividing the whole molar mass by oxygen molar mass? I'm really confused, please help!!
Asked by suzy - Fri Feb 29 20:03:44 2008 - - 2 Answers - 0 Comments
A. I'm glad you said you know how to do this. As far as doing it right, you already did. The 15 grams extra information. A teacher would probably not give you any partial credit if you used the 15 grams in a calculation. Good Job!
Answered by Derrick - Fri Feb 29 20:28:02 2008
How do you calculate the percent composition of an unknown compound?
Q. A combustion method was used to analyze a compound that was used as an additive in gasoline. A 12.069 mg sample of the compound yielded 33.652 mg of carbon dioxide and 8.123 mg of water from this reaction. Thank You!
Asked by Shazeeda - Mon Oct 19 19:55:25 2009 - - 1 Answers - 0 Comments
Q. A combustion method was used to analyze a compound that was used as an additive in gasoline. A 12.069 mg sample of the compound yielded 33.652 mg of carbon dioxide and 8.123 mg of water from this reaction. Thank You!
Asked by Shazeeda - Mon Oct 19 19:55:25 2009 - - 1 Answers - 0 Comments
What is the mass percent composition of oxygen in a compound having the empirical formula C11H18O3?
Q. Please show me how to do this I have a lot of problems like this
Asked by squirt - Thu Nov 12 19:20:03 2009 - - 4 Answers - 0 Comments
Q. Please show me how to do this I have a lot of problems like this
Asked by squirt - Thu Nov 12 19:20:03 2009 - - 4 Answers - 0 Comments
How do you find the empirical formula from the percent composition?
Q. for example: 7.8% carbon and 92.2% how would you find the empiricale formula. sorry 92.2 % chlorine
Asked by MJ149 - Wed Jan 21 00:28:19 2009 - - 2 Answers - 0 Comments
A. 7.8% Carbon and 92.2% Hydrogen Ratio of H:C= 1:12 Doesn't work, I think you got it reversed.
Answered by Crazy_Jax - Wed Jan 21 00:33:27 2009
Q. for example: 7.8% carbon and 92.2% how would you find the empiricale formula. sorry 92.2 % chlorine
Asked by MJ149 - Wed Jan 21 00:28:19 2009 - - 2 Answers - 0 Comments
A. 7.8% Carbon and 92.2% Hydrogen Ratio of H:C= 1:12 Doesn't work, I think you got it reversed.
Answered by Crazy_Jax - Wed Jan 21 00:33:27 2009
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