What is the difference between a molecular formula and an empirical formula?
Q. What is the difference between a molecular formula and an empirical formula? What is the molecular formula of the molecule that has an empirical formula of CH2O and a molar mass of 120.12 g/mol? Please help me!
Asked by Master Lee - Thu Feb 5 21:19:54 2009 - - 3 Answers - 0 Comments
A. A molecular formula tells you the ratios of each different element in a molecule. An empirical formula tells you just the lowest ratio of the different elements in each molecule. Each has a specific weight associated with it, and the molecular weight will always be a whole number multiple of the empirical weight. In this case, the empirical formula CH2O has an associated empirical weight of 12 + 2 + 16 = 30 g/equivalent. The molecular weight is (almost) exactly 4 times the empirical weight, meaning that the molecular formula is exactly four times the empirical formula: C4H8O4.
Answered by rmjrenneboog - Thu Feb 5 21:30:11 2009
Q. What is the difference between a molecular formula and an empirical formula? What is the molecular formula of the molecule that has an empirical formula of CH2O and a molar mass of 120.12 g/mol? Please help me!
Asked by Master Lee - Thu Feb 5 21:19:54 2009 - - 3 Answers - 0 Comments
A. A molecular formula tells you the ratios of each different element in a molecule. An empirical formula tells you just the lowest ratio of the different elements in each molecule. Each has a specific weight associated with it, and the molecular weight will always be a whole number multiple of the empirical weight. In this case, the empirical formula CH2O has an associated empirical weight of 12 + 2 + 16 = 30 g/equivalent. The molecular weight is (almost) exactly 4 times the empirical weight, meaning that the molecular formula is exactly four times the empirical formula: C4H8O4.
Answered by rmjrenneboog - Thu Feb 5 21:30:11 2009
What is the molecular formula for a compound with an empirical formula of NO2 and a molecular mass of 92.0?
Q. What is the molecular formula for a compound with an empirical formula of NO2 and a molecular mass of 92.0 g/mol? Thank you so much! And if it is not any trouble how do I solve this problem? 2. What is the empirical forumula for a compound if a 32.8 g sample contains 2.00 g carbon, 22.8 g of barium, and 8.00 g of oxygen? thanks so much!
Asked by Hello - Thu Dec 20 20:04:23 2007 - - 1 Answers - 0 Comments
A. 1. N2O4. You take the molar mass of NO2, 46 g/mole and then do 92/46=2. Multiply: 2(NO2) which is N2O4 2. CSO3. Take the grams of eah and divide it by the molar mass of each element. After, divide all those answers by the smalles number answer
Answered by tnpjj13 - Thu Dec 20 20:15:24 2007
Q. What is the molecular formula for a compound with an empirical formula of NO2 and a molecular mass of 92.0 g/mol? Thank you so much! And if it is not any trouble how do I solve this problem? 2. What is the empirical forumula for a compound if a 32.8 g sample contains 2.00 g carbon, 22.8 g of barium, and 8.00 g of oxygen? thanks so much!
Asked by Hello - Thu Dec 20 20:04:23 2007 - - 1 Answers - 0 Comments
A. 1. N2O4. You take the molar mass of NO2, 46 g/mole and then do 92/46=2. Multiply: 2(NO2) which is N2O4 2. CSO3. Take the grams of eah and divide it by the molar mass of each element. After, divide all those answers by the smalles number answer
Answered by tnpjj13 - Thu Dec 20 20:15:24 2007
The molecular formula mass of this compound is 240 . What are the subscripts in the actual molecular formula?
Q. The molecular formula mass of this compound is 240 . What are the subscripts in the actual molecular formula?
Asked by babyL401 - Mon Oct 5 20:20:05 2009 - - 1 Answers - 0 Comments
Q. The molecular formula mass of this compound is 240 . What are the subscripts in the actual molecular formula?
Asked by babyL401 - Mon Oct 5 20:20:05 2009 - - 1 Answers - 0 Comments
What are the molecular formula and the molar mass of the compound?
Q. Pheromones are compounds secreted by the females of many insects to attract males. One of these compounds contain 80.78% C, 13.56% H, and 5.66% O. A solution of 1 g of this pheromone in 8.50 g of benzene freezes at 3.37 degrees Celsius. What are the molecular formula and the molar mass of the compound? ( the normal freezing point of pure benzene is 5.50 degrees celsius )
Asked by Angelical Abby - Wed May 28 21:24:24 2008 - - 2 Answers - 0 Comments
A. imagine you have 100 g 80.78 g of carbon = 6.73 mol 13.56 g of H = 13.45 mol 5.66 g of O = 0.353 mol Divide all by the lowest 6.73 / 0.353 = 19 13.45 / 0.353 = 38 0.353 / 0.353 = 1 Your empirical formula is C19H38O The freezing point depression constant for benzene is 5.12 C kg/mol Your depression (ha!) is 5.50 - 3.37 = 2.13 C That means your concentration is 2.13/5.12 = 0.416 m So in 8.5 g of solvent you have 0.416 m x 0.0085 kg = 0.00354 mol 1 g / 0.00354 mol = 282 g/mol Your empirical formula weighs 12(19) + 38 + 16 = 282 So you have one empirical formula per molecular formula and your molar mass is 282.
Answered by Fly On The Wall - Wed May 28 21:40:16 2008
Q. Pheromones are compounds secreted by the females of many insects to attract males. One of these compounds contain 80.78% C, 13.56% H, and 5.66% O. A solution of 1 g of this pheromone in 8.50 g of benzene freezes at 3.37 degrees Celsius. What are the molecular formula and the molar mass of the compound? ( the normal freezing point of pure benzene is 5.50 degrees celsius )
Asked by Angelical Abby - Wed May 28 21:24:24 2008 - - 2 Answers - 0 Comments
A. imagine you have 100 g 80.78 g of carbon = 6.73 mol 13.56 g of H = 13.45 mol 5.66 g of O = 0.353 mol Divide all by the lowest 6.73 / 0.353 = 19 13.45 / 0.353 = 38 0.353 / 0.353 = 1 Your empirical formula is C19H38O The freezing point depression constant for benzene is 5.12 C kg/mol Your depression (ha!) is 5.50 - 3.37 = 2.13 C That means your concentration is 2.13/5.12 = 0.416 m So in 8.5 g of solvent you have 0.416 m x 0.0085 kg = 0.00354 mol 1 g / 0.00354 mol = 282 g/mol Your empirical formula weighs 12(19) + 38 + 16 = 282 So you have one empirical formula per molecular formula and your molar mass is 282.
Answered by Fly On The Wall - Wed May 28 21:40:16 2008
What is the molecular formula of the compound?
Q. Analysis of a newly discovered gaseous silicon-fluorine compound shows that it contains 33.01 mass % silicon. At 27 C, 2.60 g of the compound exerts a pressure of 1.50 atm in a 0.250 L vessel. What is the molecular formula of the compound? Can someone help with the steps, thanks!
Asked by shaneruzin - Mon Oct 6 10:14:30 2008 - - 3 Answers - 0 Comments
A. use PV = nRT first P = 1.5 atm V = 0.25 L T = 27 C = 300 K R = 0.08206 atm.L/K.mol n = 0.01523 mol of the compound find the molecular mass of the compound n = mass/molecular weight 0.01523 mol = 2.6 g/MW MW = 170.6848 g/mol now the tricky part the compound consists of 33.01% mass of Si means the balance of 66.99% mass is F the MW = 170.6848 g/mol then the amount of Si = 170.6848 g/mol x 0.3301 g/ (g/mol) Si = 56.343 g the amount of F = 170.6838 g/mol x 0.6699 g/ (g/mol) F = 114.342 g find the moles of each element n Si 2 n F 6 then the formula = Si2F6
Answered by pOjiE - Mon Oct 6 10:52:39 2008
Q. Analysis of a newly discovered gaseous silicon-fluorine compound shows that it contains 33.01 mass % silicon. At 27 C, 2.60 g of the compound exerts a pressure of 1.50 atm in a 0.250 L vessel. What is the molecular formula of the compound? Can someone help with the steps, thanks!
Asked by shaneruzin - Mon Oct 6 10:14:30 2008 - - 3 Answers - 0 Comments
A. use PV = nRT first P = 1.5 atm V = 0.25 L T = 27 C = 300 K R = 0.08206 atm.L/K.mol n = 0.01523 mol of the compound find the molecular mass of the compound n = mass/molecular weight 0.01523 mol = 2.6 g/MW MW = 170.6848 g/mol now the tricky part the compound consists of 33.01% mass of Si means the balance of 66.99% mass is F the MW = 170.6848 g/mol then the amount of Si = 170.6848 g/mol x 0.3301 g/ (g/mol) Si = 56.343 g the amount of F = 170.6838 g/mol x 0.6699 g/ (g/mol) F = 114.342 g find the moles of each element n Si 2 n F 6 then the formula = Si2F6
Answered by pOjiE - Mon Oct 6 10:52:39 2008
What is the molecular formula of the mystery compound?
Q. A 58.90 g sample of a mystery compound containing carbon, hydrogen, and oxygen is subjected to combustion analysis. 86.35 g CO2 and 35.35 g H2O are produced in the combustion reaction. The molar mass of the mystery compound is found to be 60.052 g/mol. What is the molecular formula of the mystery compound?
Asked by nuriiia - Sun Oct 19 10:56:55 2008 - - 1 Answers - 0 Comments
A. Moles CO2 = 86.35 g / 44.0098 g/mol = 1.962 Mass C = 1.962 mol x 12.011 g/mol = 23.57 g Moles water = 35.35 g / 18.02 g/mol = 1.962 Moles H = 2 x 1.962 = 3.924 Mass H = 1.008 g/mol x 3.924 mol = 3.955 g Mass O = 58.90 - ( 3.955 + 23.57)= 31.37 g Moles O = 31.37 g / 15.9994 g/mol =1.961 C 1.962 H 3.924 O 1.961 the empirical formula is CH2O ( molar mass = 30.0264 g/mol) 60.052 / 30.0264 = 2 multiply by 2 the empirical formula and the molecular formula is C2H4O2
Answered by Dr.A - Sun Oct 19 12:05:40 2008
Q. A 58.90 g sample of a mystery compound containing carbon, hydrogen, and oxygen is subjected to combustion analysis. 86.35 g CO2 and 35.35 g H2O are produced in the combustion reaction. The molar mass of the mystery compound is found to be 60.052 g/mol. What is the molecular formula of the mystery compound?
Asked by nuriiia - Sun Oct 19 10:56:55 2008 - - 1 Answers - 0 Comments
A. Moles CO2 = 86.35 g / 44.0098 g/mol = 1.962 Mass C = 1.962 mol x 12.011 g/mol = 23.57 g Moles water = 35.35 g / 18.02 g/mol = 1.962 Moles H = 2 x 1.962 = 3.924 Mass H = 1.008 g/mol x 3.924 mol = 3.955 g Mass O = 58.90 - ( 3.955 + 23.57)= 31.37 g Moles O = 31.37 g / 15.9994 g/mol =1.961 C 1.962 H 3.924 O 1.961 the empirical formula is CH2O ( molar mass = 30.0264 g/mol) 60.052 / 30.0264 = 2 multiply by 2 the empirical formula and the molecular formula is C2H4O2
Answered by Dr.A - Sun Oct 19 12:05:40 2008
What is the molecular formula of vanilla according to the given information?
Q. Vanillin is a compound that is used as a flavoring agent in many food products. Vanilla is 63.2% Carbon, 5.3% Hydrogen, and 31.5% Oxygen. The molar mass is approximately 152 grams per mole. What is the molecular formula for vanilla?
Asked by Melabuu - Thu Apr 9 00:10:35 2009 - - 1 Answers - 0 Comments
A. moles C = 63.2 / 12.011 g/mol= 5.26 moles H = 5.3 / 1.008 g/mol= 5.26 moles O= 31.5 / 15.999 g/mol=1.97 5.26 / 1.97 = 2.7 => C = H 1.97 / 1.97 = 1 = O to get whole numbers multiply by 3 C8H8O3 empirical formula ( MM = 152 g/mol) it is also the molecular formula
Answered by Dr.A - Thu Apr 9 13:09:43 2009
Q. Vanillin is a compound that is used as a flavoring agent in many food products. Vanilla is 63.2% Carbon, 5.3% Hydrogen, and 31.5% Oxygen. The molar mass is approximately 152 grams per mole. What is the molecular formula for vanilla?
Asked by Melabuu - Thu Apr 9 00:10:35 2009 - - 1 Answers - 0 Comments
A. moles C = 63.2 / 12.011 g/mol= 5.26 moles H = 5.3 / 1.008 g/mol= 5.26 moles O= 31.5 / 15.999 g/mol=1.97 5.26 / 1.97 = 2.7 => C = H 1.97 / 1.97 = 1 = O to get whole numbers multiply by 3 C8H8O3 empirical formula ( MM = 152 g/mol) it is also the molecular formula
Answered by Dr.A - Thu Apr 9 13:09:43 2009
How do you find the molecular formula of a hydrate?
Q. I need to find the molecular formula of CuSO4 xH20. If anyone could tell me how to find the formula or link me to a site which would show me how, I'd be very thankful.
Asked by Oxide - Sun Nov 8 18:59:52 2009 - - 0 Answers - 0 Comments
Q. I need to find the molecular formula of CuSO4 xH20. If anyone could tell me how to find the formula or link me to a site which would show me how, I'd be very thankful.
Asked by Oxide - Sun Nov 8 18:59:52 2009 - - 0 Answers - 0 Comments
What is the molecular formula of kethoxal?
Q. Kethoxal, a substance use to combat viruses, is 48.6% carbon, 8.17% hydrogen, and 43.2% oxygen. It has a molar mass of 148 g/mol. What is the molecular formula of kethoxal? Any help would be appreciated, thanks.
Asked by Sciguy - Mon Oct 13 03:41:50 2008 - - 3 Answers - 0 Comments
A. Firstly find the mass each element takes up of the total molar mass: Carbon: 48.6% x 148g/mol = 71.928g Oxygen: 43.2% x 148g/mol = 63.936g Hydrogen: 8.17% x 148g/mol = 12.09g Now divide each mass by the elements molar mass: Carbon: 71.928g / 12 = 5.994 or 6 carbon atoms Oxygen: 63.936g / 16 = 3.996 or 4 oxygen atoms Hydrogen: 12.09g / 1 = 12.09 or 12 hydrogen atoms Therefore the molecular formula of Kethoxal is C6H12O4
Answered by Goddord - Mon Oct 13 04:17:51 2008
Q. Kethoxal, a substance use to combat viruses, is 48.6% carbon, 8.17% hydrogen, and 43.2% oxygen. It has a molar mass of 148 g/mol. What is the molecular formula of kethoxal? Any help would be appreciated, thanks.
Asked by Sciguy - Mon Oct 13 03:41:50 2008 - - 3 Answers - 0 Comments
A. Firstly find the mass each element takes up of the total molar mass: Carbon: 48.6% x 148g/mol = 71.928g Oxygen: 43.2% x 148g/mol = 63.936g Hydrogen: 8.17% x 148g/mol = 12.09g Now divide each mass by the elements molar mass: Carbon: 71.928g / 12 = 5.994 or 6 carbon atoms Oxygen: 63.936g / 16 = 3.996 or 4 oxygen atoms Hydrogen: 12.09g / 1 = 12.09 or 12 hydrogen atoms Therefore the molecular formula of Kethoxal is C6H12O4
Answered by Goddord - Mon Oct 13 04:17:51 2008
What is the molecular formula of this gas?
Q. Lab technicians determine that a gas collected from a marshy area is made up of 80.0% carbon and 20.0% hydrogen. They also find that a 4.50g sample occupies a volume of 3.44L at STP. What is the molecular formula of this gas?
Asked by pumpkinpie - Mon Nov 2 07:27:30 2009 - - 1 Answers - 0 Comments
A. Use the ideal gas law. Isolate molar mass in the formula. PV = nRT PV = (mass / molar mass)RT PV / RT = mass / molar mass molar mass = mass / (PV / RT) molar mass = 4.50 g / ([1 atm][3.44 L] / [0.0821][273 K]) molar mass = 29.32 g/mol Let's leave this for now and determine the empirical formula. Find the number of moles of each element involved in the compound. Let our compound's mass be 100 g. C: 80.0 g / 12.011 g/mol = 6.67 mol H: 20.0 g / 1.01 g/mol = 19.8 mol Divide both values by the lowest value: 6.67 C: 6.67 / 6.67 = 1 H: 19.8 / 6.67 = 3 Empirical formula: CH Calculate the molecular formula. = actual molar mass / emp. molar mass = 29.32 g/mol / 15.03 g/mol = 2 Multiply the empirical formula by 2. molecular formula = 2(CH )… [cont.]
Answered by Dr. Lucafont - Mon Nov 2 07:49:09 2009
Q. Lab technicians determine that a gas collected from a marshy area is made up of 80.0% carbon and 20.0% hydrogen. They also find that a 4.50g sample occupies a volume of 3.44L at STP. What is the molecular formula of this gas?
Asked by pumpkinpie - Mon Nov 2 07:27:30 2009 - - 1 Answers - 0 Comments
A. Use the ideal gas law. Isolate molar mass in the formula. PV = nRT PV = (mass / molar mass)RT PV / RT = mass / molar mass molar mass = mass / (PV / RT) molar mass = 4.50 g / ([1 atm][3.44 L] / [0.0821][273 K]) molar mass = 29.32 g/mol Let's leave this for now and determine the empirical formula. Find the number of moles of each element involved in the compound. Let our compound's mass be 100 g. C: 80.0 g / 12.011 g/mol = 6.67 mol H: 20.0 g / 1.01 g/mol = 19.8 mol Divide both values by the lowest value: 6.67 C: 6.67 / 6.67 = 1 H: 19.8 / 6.67 = 3 Empirical formula: CH Calculate the molecular formula. = actual molar mass / emp. molar mass = 29.32 g/mol / 15.03 g/mol = 2 Multiply the empirical formula by 2. molecular formula = 2(CH )… [cont.]
Answered by Dr. Lucafont - Mon Nov 2 07:49:09 2009
What is the molecular formula of this aromatic compound?
Q. The density is 1.16g/dm3 aromatic compound is 92.3% C and 7.7 H by mass. What is the molecular formula of this aromatic compound? Have no idea what i have to do with density. Any help is appreciated! Thanks.
Asked by Karmo - Wed Oct 21 05:22:08 2009 - - 2 Answers - 0 Comments
A. We accept that the empirical formula is CH Now to solve the (apparent) density problem From the low density, the compound is a gas. 1 mol of a gas at STP has volume 22.4 litres Therefore the unknown gas will have molar mass= 22.4*1.16 = 25.984g/mol CH = 12.+1 = 13 g/ formula 25.984 / 13. = 2 Molecular formula = (CH)2 = C2H2 = ethyne. Edit Later: I reread your question: are you sure the question said aromatic compound? Ethyne is not an aromatic. I do not know that it is possible for an aromatic to be a gas with a density of 1.16 g/dm . In fact I am convinced that it is impossible.
Answered by Trevor H - Wed Oct 21 08:18:46 2009
Q. The density is 1.16g/dm3 aromatic compound is 92.3% C and 7.7 H by mass. What is the molecular formula of this aromatic compound? Have no idea what i have to do with density. Any help is appreciated! Thanks.
Asked by Karmo - Wed Oct 21 05:22:08 2009 - - 2 Answers - 0 Comments
A. We accept that the empirical formula is CH Now to solve the (apparent) density problem From the low density, the compound is a gas. 1 mol of a gas at STP has volume 22.4 litres Therefore the unknown gas will have molar mass= 22.4*1.16 = 25.984g/mol CH = 12.+1 = 13 g/ formula 25.984 / 13. = 2 Molecular formula = (CH)2 = C2H2 = ethyne. Edit Later: I reread your question: are you sure the question said aromatic compound? Ethyne is not an aromatic. I do not know that it is possible for an aromatic to be a gas with a density of 1.16 g/dm . In fact I am convinced that it is impossible.
Answered by Trevor H - Wed Oct 21 08:18:46 2009
What is the molecular formula of the alcohol?
Q. An alcohol is 64.81% C, 13.60% H, and 21.59%. O by mass. Another experiment shows that its l11ol~cu'ar weight is approximately 74 amu. What is the molecular formula of the alcohol?
Asked by mohamed r - Fri Nov 23 17:20:11 2007 - - 3 Answers - 0 Comments
A. To solve these, first divide the weight % by the atomic weight to get relative amounts by numbers of atoms. 64.81/12.01 = 5.396 13.60/1.01 = 13.46 21.59/16.00 = 1.349 These values are proportional to the formula, but we need to get this into whole numbers. Let's try dividing them by the smallest number (its a good staring point). 5.396/1.349 = 4.00 13.46/1.349 = 9.978 1.349/1.349 = 1 These valuse are close enough to whole numbers to be OK; now, we have what is called an empirical formula: C4H10O. This may, or may not be the actual formula. The actual formula could be a multiple of this. Now, let's see what the empirical formula weighs: (12.01 x 4) + (1.01 x 10) + 16.00 = 74.14g Since the molecular weight was already determined to be ~ [cont.]
Answered by Flying Dragon - Fri Nov 23 17:44:06 2007
Q. An alcohol is 64.81% C, 13.60% H, and 21.59%. O by mass. Another experiment shows that its l11ol~cu'ar weight is approximately 74 amu. What is the molecular formula of the alcohol?
Asked by mohamed r - Fri Nov 23 17:20:11 2007 - - 3 Answers - 0 Comments
A. To solve these, first divide the weight % by the atomic weight to get relative amounts by numbers of atoms. 64.81/12.01 = 5.396 13.60/1.01 = 13.46 21.59/16.00 = 1.349 These values are proportional to the formula, but we need to get this into whole numbers. Let's try dividing them by the smallest number (its a good staring point). 5.396/1.349 = 4.00 13.46/1.349 = 9.978 1.349/1.349 = 1 These valuse are close enough to whole numbers to be OK; now, we have what is called an empirical formula: C4H10O. This may, or may not be the actual formula. The actual formula could be a multiple of this. Now, let's see what the empirical formula weighs: (12.01 x 4) + (1.01 x 10) + 16.00 = 74.14g Since the molecular weight was already determined to be ~ [cont.]
Answered by Flying Dragon - Fri Nov 23 17:44:06 2007
What is the molecular formula if its molar mass is aproxumately 121g?
Q. the percent composition of cysteine is 29.74% C, 5.82% H, 26.41% O, 11.56% N, 26.47% S. What is the molecular formula it its molar mass is approximately 121g?
Asked by Tim - Mon Oct 26 12:09:44 2009 - - 1 Answers - 0 Comments
A. assume 100g... moles C = 29.74g x (1 mole / 12.01g) = 2.476 moles H = 5.82g x (1 mole / 1.008g) = 5.774 moles O = 26.41g x (1 mole / 16.00g) = 1.651 moles N = 11.56g x (1 mole / 14.01g) = 0.8251 moles S = 26.47g x (1 mole / 32.07g) = 0.8253 now we simply those #'s by dividing all by the smallest. that forces at least 1 # to = 1 and the rest to be > 1 moles C = 2.476 / 0.8251 = 3 moles H = 5.774 / 0.8251 = 7 moles O = 1.651 / 0.8251 = 2 moles N = 0.8251 / 0.8251 = 1 moles S = 0.8253 / 0.8251 = 1 and your empirical formula is C3H7O2NS.. and that has empirical mass = 121 g/unit so there must be 1 unit per molecule. and your molecular formula is C3H7NO2S *** alternately... you could start with 121g... and skip the empirical formula… [cont.]
Answered by m w - Mon Oct 26 12:32:41 2009
Q. the percent composition of cysteine is 29.74% C, 5.82% H, 26.41% O, 11.56% N, 26.47% S. What is the molecular formula it its molar mass is approximately 121g?
Asked by Tim - Mon Oct 26 12:09:44 2009 - - 1 Answers - 0 Comments
A. assume 100g... moles C = 29.74g x (1 mole / 12.01g) = 2.476 moles H = 5.82g x (1 mole / 1.008g) = 5.774 moles O = 26.41g x (1 mole / 16.00g) = 1.651 moles N = 11.56g x (1 mole / 14.01g) = 0.8251 moles S = 26.47g x (1 mole / 32.07g) = 0.8253 now we simply those #'s by dividing all by the smallest. that forces at least 1 # to = 1 and the rest to be > 1 moles C = 2.476 / 0.8251 = 3 moles H = 5.774 / 0.8251 = 7 moles O = 1.651 / 0.8251 = 2 moles N = 0.8251 / 0.8251 = 1 moles S = 0.8253 / 0.8251 = 1 and your empirical formula is C3H7O2NS.. and that has empirical mass = 121 g/unit so there must be 1 unit per molecule. and your molecular formula is C3H7NO2S *** alternately... you could start with 121g... and skip the empirical formula… [cont.]
Answered by m w - Mon Oct 26 12:32:41 2009
What is the difference between a chemical formula and a molecular formula?
Q. im pretty sure a molecular formula is a chemical formula for a molecular compound, but a molecular formula is not a chemical formula unless it is for a molecular compound...i think...idk im really confused haha
Asked by Bailey Bean - Sat Oct 17 21:17:53 2009 - - 1 Answers - 0 Comments
Q. im pretty sure a molecular formula is a chemical formula for a molecular compound, but a molecular formula is not a chemical formula unless it is for a molecular compound...i think...idk im really confused haha
Asked by Bailey Bean - Sat Oct 17 21:17:53 2009 - - 1 Answers - 0 Comments
What is the molecular formula for glucose?
Q. Glucose contains the elements C, H, and O. It is known to contain 40.0% C and 6.71% H by mass. The molecular weight of glucose has been found to be about 180.16 g/mol. What is the molecular formula for glucose?
Asked by JohnD - Thu Apr 16 11:08:56 2009 - - 1 Answers - 0 Comments
A. 0.40 x 180.16 = 72.064g / 12.010C = C 6 0.0671 x 180.16 = 12.089 / 1 = H 12 0.533 x 180.16 = 96.025 / 16 = O 6 C6H12O6
Answered by unknown - Thu Apr 16 13:40:17 2009
Q. Glucose contains the elements C, H, and O. It is known to contain 40.0% C and 6.71% H by mass. The molecular weight of glucose has been found to be about 180.16 g/mol. What is the molecular formula for glucose?
Asked by JohnD - Thu Apr 16 11:08:56 2009 - - 1 Answers - 0 Comments
A. 0.40 x 180.16 = 72.064g / 12.010C = C 6 0.0671 x 180.16 = 12.089 / 1 = H 12 0.533 x 180.16 = 96.025 / 16 = O 6 C6H12O6
Answered by unknown - Thu Apr 16 13:40:17 2009
How do you solve a molecular formula problem?
Q. I do not know how to solve these two problems and I cant seem to find anything that explains it well. Help please.. A sample of a compound with a formula mass of 34.00 amu is found to consist of 0.44g H and 6.92g O. Find its molecular formula. and.. If 4.04g ofN combine with 11.46g of O to produce a compound with a formula mass of 108.0 amu, what is the molecular formula of this compound?
Asked by surfergrly12 - Sun Aug 30 16:55:53 2009 - - 1 Answers - 0 Comments
A. H2O2 N2O5 Convert N, H, and O weights to moles and take the ratio of each to the other.
Answered by jerry758 - Sun Aug 30 17:04:55 2009
Q. I do not know how to solve these two problems and I cant seem to find anything that explains it well. Help please.. A sample of a compound with a formula mass of 34.00 amu is found to consist of 0.44g H and 6.92g O. Find its molecular formula. and.. If 4.04g ofN combine with 11.46g of O to produce a compound with a formula mass of 108.0 amu, what is the molecular formula of this compound?
Asked by surfergrly12 - Sun Aug 30 16:55:53 2009 - - 1 Answers - 0 Comments
A. H2O2 N2O5 Convert N, H, and O weights to moles and take the ratio of each to the other.
Answered by jerry758 - Sun Aug 30 17:04:55 2009
How to deduce molecular formula of isomers?
Q. My question is: Butane was reacted with chlorine to form a mixture of isomers. Two isomers A and B were separated from this mixture. These isomers had a molar mass of 92.5 g mol-1. Deduce the molecular formula of these two isomers. Second part of question: draw the displayed formulae of A and B and name each compound. I thought that the fact that it reacted with chlorine meant that it was free radical substitution. But that doesn't form isomers does it? What's the answer please... and how to get there.
Asked by aadam_hashmi - Wed Mar 19 17:41:10 2008 - - 1 Answers - 0 Comments
A. This molecular mass means that a single hydrogen has been replaced by a single chlorine atom. You're forming chlorobutane. Because of the structure, the isomers are 1-chlorobutane and 2-chlorobutane. The condensed formulae are: Cl-CH2-CH2-CH2-CH3 (1-chloro) and CH3-CHCl-CH2-CH3 (2-chloro). Hope that helps.
Answered by kumorifox - Wed Mar 19 18:03:15 2008
Q. My question is: Butane was reacted with chlorine to form a mixture of isomers. Two isomers A and B were separated from this mixture. These isomers had a molar mass of 92.5 g mol-1. Deduce the molecular formula of these two isomers. Second part of question: draw the displayed formulae of A and B and name each compound. I thought that the fact that it reacted with chlorine meant that it was free radical substitution. But that doesn't form isomers does it? What's the answer please... and how to get there.
Asked by aadam_hashmi - Wed Mar 19 17:41:10 2008 - - 1 Answers - 0 Comments
A. This molecular mass means that a single hydrogen has been replaced by a single chlorine atom. You're forming chlorobutane. Because of the structure, the isomers are 1-chlorobutane and 2-chlorobutane. The condensed formulae are: Cl-CH2-CH2-CH2-CH3 (1-chloro) and CH3-CHCl-CH2-CH3 (2-chloro). Hope that helps.
Answered by kumorifox - Wed Mar 19 18:03:15 2008
what is the molecular formula of styrene?
Q. Styrene has 92.26% of Carbon and 7.74% of Hydrogen. Further experimentation determines that the molecular weight of this compound is 78.11 grams per mole. What is the molecular formula of styrene? btw, if someone could generally state how to find the molecular formula, it would be really helpful. I understand how to find empirical formulas but i don't understand how to find the molecular formulas..
Asked by Mango - Sun Sep 23 03:17:47 2007 - - 3 Answers - 0 Comments
A. No of mol of each element = percentage by mass / molar mass C: 92.26 / 12.0 = 7.689 H: 7.74 / 1.0 = 7.74 Simplest mole ratio C: 1 , H: 1 Empirical formula of styrene = CH Molecular formula = (empirical formula)n, where n = Molar mass of molecular formula / mass of empirical formula. n = 78.11/(1.0 + 12.0) = 6 Hence, molecular formula: C6H6 However, the molar mass given in the question appears to be wrong, since the molar mass of styrene is 104.15 g/mol. C6H6 is the molecular formula of benzene.
Answered by Huppiness - Sun Sep 23 03:33:09 2007
Q. Styrene has 92.26% of Carbon and 7.74% of Hydrogen. Further experimentation determines that the molecular weight of this compound is 78.11 grams per mole. What is the molecular formula of styrene? btw, if someone could generally state how to find the molecular formula, it would be really helpful. I understand how to find empirical formulas but i don't understand how to find the molecular formulas..
Asked by Mango - Sun Sep 23 03:17:47 2007 - - 3 Answers - 0 Comments
A. No of mol of each element = percentage by mass / molar mass C: 92.26 / 12.0 = 7.689 H: 7.74 / 1.0 = 7.74 Simplest mole ratio C: 1 , H: 1 Empirical formula of styrene = CH Molecular formula = (empirical formula)n, where n = Molar mass of molecular formula / mass of empirical formula. n = 78.11/(1.0 + 12.0) = 6 Hence, molecular formula: C6H6 However, the molar mass given in the question appears to be wrong, since the molar mass of styrene is 104.15 g/mol. C6H6 is the molecular formula of benzene.
Answered by Huppiness - Sun Sep 23 03:33:09 2007
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 molecular formula for this gas ?
Q. For a certain gas that contains only carbon and hydrogen the mass percentage of carbon is known to be 85.62. It is also known that 2.55 g of the gas has a volume of 1.00 L and a pressure of 0.970 atm at 51.6 oC. What is the molecular formula for the gas ?
Asked by jessica c - Sun Mar 30 23:41:50 2008 - - 1 Answers - 0 Comments
A. PV = nRT n = PV/RT n = (0.970atm)(1.00L)/ (0.08206Latm/molK)(324.6K ) n = 0.0364 mol molecular mass of the gas 2.55 g / 0.0364 mol = 70.0 g / mol the molecular mass of total carbon in gas 70.0g/mol * 0.8562 = 59.95 g/mol carbon atoms 59.95 g/mol divided by 12.01g/mol (that is a single carbon) = 5 molecular mass of hydrogen atoms = 70.0 g/mol - 59.95 g/mol = ~10 g/mol therefore, 10 H atoms molecular formula is C5H10
Answered by roflguy - Sun Mar 30 23:45:17 2008
Q. For a certain gas that contains only carbon and hydrogen the mass percentage of carbon is known to be 85.62. It is also known that 2.55 g of the gas has a volume of 1.00 L and a pressure of 0.970 atm at 51.6 oC. What is the molecular formula for the gas ?
Asked by jessica c - Sun Mar 30 23:41:50 2008 - - 1 Answers - 0 Comments
A. PV = nRT n = PV/RT n = (0.970atm)(1.00L)/ (0.08206Latm/molK)(324.6K ) n = 0.0364 mol molecular mass of the gas 2.55 g / 0.0364 mol = 70.0 g / mol the molecular mass of total carbon in gas 70.0g/mol * 0.8562 = 59.95 g/mol carbon atoms 59.95 g/mol divided by 12.01g/mol (that is a single carbon) = 5 molecular mass of hydrogen atoms = 70.0 g/mol - 59.95 g/mol = ~10 g/mol therefore, 10 H atoms molecular formula is C5H10
Answered by roflguy - Sun Mar 30 23:45:17 2008
From Yahoo Answer Search: 'molecular formula'
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Do you know the Molecular Formula of your compound Step 1 The Sadtler indexes on are on the Chemistry Table look for the blue volumes marked 1980 Cumulative Molecular Formula Index Look up the molecular formula
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Structural isomers: is a form of isomerism in which molecules with the same . molecular formula. have atoms bonded together in different orders, as opposed to stereoisomerism. 4. Geometric isomers: one of several compounds that have the ...
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