Molecular formula for caffeine?
Q. I know that the molecular formula will turn out to be C8H10N4O2 because I've looked it up. But how would you determine the moelcular formula knowing the empirical fomula (C4H5N2O) and that the molar mass of caffeine is 195 g/mol?
Asked by osnap.itstom - Mon Apr 7 00:57:57 2008 - - 2 Answers - 0 Comments
A. Divide the molar mass of coffiene by the molar mass of the empirical formula and multiply the subscripts of the empirical formula by that numbber
Answered by Sly_Salmon - Mon Apr 7 01:01:40 2008
Q. I know that the molecular formula will turn out to be C8H10N4O2 because I've looked it up. But how would you determine the moelcular formula knowing the empirical fomula (C4H5N2O) and that the molar mass of caffeine is 195 g/mol?
Asked by osnap.itstom - Mon Apr 7 00:57:57 2008 - - 2 Answers - 0 Comments
A. Divide the molar mass of coffiene by the molar mass of the empirical formula and multiply the subscripts of the empirical formula by that numbber
Answered by Sly_Salmon - Mon Apr 7 01:01:40 2008
What is the empirical formula of Caffeine?
Q. The molecular formula is C8H10N4O2...I got C4H5N2O, is that right?
Asked by ? - Mon Sep 14 23:49:14 2009 - - 1 Answers - 0 Comments
A. Yes, the empirical formula is just molecular formula reduced to the smallest whole numbers.
Answered by Flying Dragon - Tue Sep 15 00:06:26 2009
Q. The molecular formula is C8H10N4O2...I got C4H5N2O, is that right?
Asked by ? - Mon Sep 14 23:49:14 2009 - - 1 Answers - 0 Comments
A. Yes, the empirical formula is just molecular formula reduced to the smallest whole numbers.
Answered by Flying Dragon - Tue Sep 15 00:06:26 2009
The empirical and molecular formula...?
Q. Determine the empirical and molecular formula a)caffeine, a stimulant found in coffee, contains 49.5 percent C, 5.15 percent H, 28.9 percent N, and 16.5 percent O by mass; molar mass about 195g b)Modosodium glotamate, a flavor enhancer in certain foods contains 35.51 percent C, 4.77 percent H, 37.85 percent O, 8.29 percent N and 13.60 percent Na and has a molar mass of 169g Thank you for your time 10 points
Asked by pianoman3434 - Sat Aug 16 20:16:28 2008 - - 1 Answers - 0 Comments
A. a) Assume that we have 100 g of caffeine. Based on the percentages given, we have 49.5 g C, 5.15 g H, 28.9 g N, and 16.5 g O. We need to calculate moles of each. C: 49.5 g / 12.0 g/mole = 4.13 moles C H: 5.15 g / 1.01 g/mole = 5.10 moles H N: 28.9 g / 14.0 g/mole = 2.06 moles N O: 16.5 g / 16.0 g/mole = 1.03 moles O Dividing by the smallest (1.03) we get C - 4 H - 5 N - 2 O - 1 The empirical formula is C4H5N2O. Its formula weight is (4 x 12) + (5 x 1) + (2 x 14) + (1 x 16) = 97. If the molar mass is 195, that's equal to 2 empirical formula units (2 x 97 = 194). So the molecular formula is 2 x C4H5N2O = C8H10N4O2. b) Work this exactly like the one above. You should get a molecular formula of C5H8O4NNa.
Answered by HPV - Sat Aug 16 20:35:17 2008
Q. Determine the empirical and molecular formula a)caffeine, a stimulant found in coffee, contains 49.5 percent C, 5.15 percent H, 28.9 percent N, and 16.5 percent O by mass; molar mass about 195g b)Modosodium glotamate, a flavor enhancer in certain foods contains 35.51 percent C, 4.77 percent H, 37.85 percent O, 8.29 percent N and 13.60 percent Na and has a molar mass of 169g Thank you for your time 10 points
Asked by pianoman3434 - Sat Aug 16 20:16:28 2008 - - 1 Answers - 0 Comments
A. a) Assume that we have 100 g of caffeine. Based on the percentages given, we have 49.5 g C, 5.15 g H, 28.9 g N, and 16.5 g O. We need to calculate moles of each. C: 49.5 g / 12.0 g/mole = 4.13 moles C H: 5.15 g / 1.01 g/mole = 5.10 moles H N: 28.9 g / 14.0 g/mole = 2.06 moles N O: 16.5 g / 16.0 g/mole = 1.03 moles O Dividing by the smallest (1.03) we get C - 4 H - 5 N - 2 O - 1 The empirical formula is C4H5N2O. Its formula weight is (4 x 12) + (5 x 1) + (2 x 14) + (1 x 16) = 97. If the molar mass is 195, that's equal to 2 empirical formula units (2 x 97 = 194). So the molecular formula is 2 x C4H5N2O = C8H10N4O2. b) Work this exactly like the one above. You should get a molecular formula of C5H8O4NNa.
Answered by HPV - Sat Aug 16 20:35:17 2008
How would you do this chemistry problem?
Q. A molecule of caffeine contains 8 carbon atoms, 10 hydrogen atoms, 4 nitrogen atoms, and 2 oxygen atoms. Determine the empirical and molecular formula for caffeine.
Asked by unknown - Sun Nov 15 18:57:57 2009 - - 2 Answers - 0 Comments
Q. A molecule of caffeine contains 8 carbon atoms, 10 hydrogen atoms, 4 nitrogen atoms, and 2 oxygen atoms. Determine the empirical and molecular formula for caffeine.
Asked by unknown - Sun Nov 15 18:57:57 2009 - - 2 Answers - 0 Comments
please help me..The stimulant in coffee and tea is caffeine, a substance of molar mass 194g/mol.?
Q. when 0.376g of caffeine was burned, 0.682g carbon dioxide, 0.174g of water and 0.110g of nitrogen were formed. determine teh empirical and molecular formulas of caffeine.. im realy confuse.
Asked by Rubieanne - Sun Apr 22 02:23:14 2007 - - 1 Answers - 0 Comments
A. Let Caffeine be CxHyOzNs where x,y,z and s have to be determined. Moles of Caffeine = 0.376/194 Moles of N2 = 0.11/28 Thus 0.376*s/(194*2) = 0.11/28 So, s = 4 Now, Moles of CO2 released = 0.376x/194 = 0.682/44 So, x = 8 Moles of H2O = 0.376*y/388 = 0.174/18 So, y = 10 Mass of O = 194-(4*14+8*12+10) = 32 g So, z = 2 Molecular formula is C8H10O2N4 and empirical formula is C4H5ON2
Answered by ag_iitkgp - Sun Apr 22 02:50:18 2007
Q. when 0.376g of caffeine was burned, 0.682g carbon dioxide, 0.174g of water and 0.110g of nitrogen were formed. determine teh empirical and molecular formulas of caffeine.. im realy confuse.
Asked by Rubieanne - Sun Apr 22 02:23:14 2007 - - 1 Answers - 0 Comments
A. Let Caffeine be CxHyOzNs where x,y,z and s have to be determined. Moles of Caffeine = 0.376/194 Moles of N2 = 0.11/28 Thus 0.376*s/(194*2) = 0.11/28 So, s = 4 Now, Moles of CO2 released = 0.376x/194 = 0.682/44 So, x = 8 Moles of H2O = 0.376*y/388 = 0.174/18 So, y = 10 Mass of O = 194-(4*14+8*12+10) = 32 g So, z = 2 Molecular formula is C8H10O2N4 and empirical formula is C4H5ON2
Answered by ag_iitkgp - Sun Apr 22 02:50:18 2007
Can anyone help me with these Chemistry questions?
Q. ...PLEASE!!! I have been working on them for 2 hours now, and I just don't understand them! What is the empirical formula of C6H12? A compound is analyzed and is found to contain 5.657 g C; 0.3165 g H; and 5.566 g Cl. What is the empirical formula? A 2.573 g oxide of iron conatins 2.000 g iron. What is its empirical formula? Caffeine is a compound containing carbon, hydrogen, nitrogen and oxygen. The percent composition of carbon is 49.47% C, 5.191% H, 28.86% N, and 16.48% oxygen. The molar mass of caffeine is approximately 194 g. What is the molecular formula of caffeine? A compound is 25.94% nitrogen and 74.06% oxygen. What is the empirical formula of the compound?
Asked by ~*PrInCeSs*~ - Sun Feb 24 12:54:02 2008 - - 1 Answers - 0 Comments
A. For question 2 it is just the least amount of C and H which can maintain the right stoichiometric equivalents for the molecule or CH2 For question 2 what you want to do first is find out how many moles of each element there are C= 5.657g /(1 mole C/12.0107g)= 0.471 moles C H= 0.3165g/(1 mole H/1.00794g)= 0.316 moles H Cl= 5.566g/(1 mole Cl/35.453g)= 0.157 moles Cl Now which one is limiting? Cl is, divide each one by # moles of Cl So C is 0.471 moles/0.157 =3 H is 0.316/0.157=2 Cl is 0.157/0.157=1 So your empirical formula is C3H2Cl Now for question 3 We know 2.000 grams is iron so 0.573 must be Oxygen. Know that we know the grams repeat the steps above. For question 4 Multiply each % by the molecular weight (194g) … [cont.]
Answered by Zachary P - Sun Feb 24 13:21:17 2008
Q. ...PLEASE!!! I have been working on them for 2 hours now, and I just don't understand them! What is the empirical formula of C6H12? A compound is analyzed and is found to contain 5.657 g C; 0.3165 g H; and 5.566 g Cl. What is the empirical formula? A 2.573 g oxide of iron conatins 2.000 g iron. What is its empirical formula? Caffeine is a compound containing carbon, hydrogen, nitrogen and oxygen. The percent composition of carbon is 49.47% C, 5.191% H, 28.86% N, and 16.48% oxygen. The molar mass of caffeine is approximately 194 g. What is the molecular formula of caffeine? A compound is 25.94% nitrogen and 74.06% oxygen. What is the empirical formula of the compound?
Asked by ~*PrInCeSs*~ - Sun Feb 24 12:54:02 2008 - - 1 Answers - 0 Comments
A. For question 2 it is just the least amount of C and H which can maintain the right stoichiometric equivalents for the molecule or CH2 For question 2 what you want to do first is find out how many moles of each element there are C= 5.657g /(1 mole C/12.0107g)= 0.471 moles C H= 0.3165g/(1 mole H/1.00794g)= 0.316 moles H Cl= 5.566g/(1 mole Cl/35.453g)= 0.157 moles Cl Now which one is limiting? Cl is, divide each one by # moles of Cl So C is 0.471 moles/0.157 =3 H is 0.316/0.157=2 Cl is 0.157/0.157=1 So your empirical formula is C3H2Cl Now for question 3 We know 2.000 grams is iron so 0.573 must be Oxygen. Know that we know the grams repeat the steps above. For question 4 Multiply each % by the molecular weight (194g) … [cont.]
Answered by Zachary P - Sun Feb 24 13:21:17 2008
CH4 is methane, there is no name but that it is a methyl group with an unpaired electron.?
Q. CH3- is a partial moleculewhich is usually part of an aromatic hydrocarbon or also found in the molecular formula for chocolate and caffeine.
Asked by unknown - Tue Jul 7 13:56:16 2009 - - 1 Answers - 0 Comments
A. It is not quite clear what your question is. Here are some suggestions. Methane, CH4, is a compound that is common in natural gas. Methyl radical can refer to .CH3, a short-lived free radical that is thought to occur as an unstable intermediate structure in reaction mechanisms such as the free-radical chlorination of methane. Methyl radical is also used in an older nomenclature to describe a CH3 bonded as a branch to some chain or ring such as you mention. Nowadays, this is more commonly referred to as a methyl group to distinguish it from .CH3.
Answered by Buck - Tue Jul 7 14:14:18 2009
Q. CH3- is a partial moleculewhich is usually part of an aromatic hydrocarbon or also found in the molecular formula for chocolate and caffeine.
Asked by unknown - Tue Jul 7 13:56:16 2009 - - 1 Answers - 0 Comments
A. It is not quite clear what your question is. Here are some suggestions. Methane, CH4, is a compound that is common in natural gas. Methyl radical can refer to .CH3, a short-lived free radical that is thought to occur as an unstable intermediate structure in reaction mechanisms such as the free-radical chlorination of methane. Methyl radical is also used in an older nomenclature to describe a CH3 bonded as a branch to some chain or ring such as you mention. Nowadays, this is more commonly referred to as a methyl group to distinguish it from .CH3.
Answered by Buck - Tue Jul 7 14:14:18 2009
I need help with my chemistry please.?
Q. Here is my problem I need help with. Caffeine, a stimulant found in coffee and soda pop, has the following mass percent composition: C, 49.48%; H, 5.19%; N, 28.85%; O, 16.48%. The molar mass of the caffeine is 194.19g/mol. Find the molecular formula of caffeine.
Asked by mjhappy17 - Sun Nov 1 13:22:29 2009 - - 6 Answers - 0 Comments
A. First establish that your going to measure using 1 mole So now you have 194.19g caffeine Carbon is 49.48% of the mass so you have (49.48%)*(194.19)=96.0852 g carbon to see how many carbons you have you do (mass/Molar mass) (96.0852/12.0107) = 10 So you have 10 carbons Do it for each one: Hydrogen: (5.19%)*(194.19) = 10.0785 g (mass/molar mass) (10.0785/1.00794) = 10 Nitrogen: (28.85%)(194.19) = 56.0238 g (56.0238/14.00674) = 4 Oxygen: (16.48%)(194.19) = 32.0025g (32.0025/15.9994) = 2 Final formula: C8 H10 N4 O2
Answered by sambkup - Sun Nov 1 13:44:10 2009
Q. Here is my problem I need help with. Caffeine, a stimulant found in coffee and soda pop, has the following mass percent composition: C, 49.48%; H, 5.19%; N, 28.85%; O, 16.48%. The molar mass of the caffeine is 194.19g/mol. Find the molecular formula of caffeine.
Asked by mjhappy17 - Sun Nov 1 13:22:29 2009 - - 6 Answers - 0 Comments
A. First establish that your going to measure using 1 mole So now you have 194.19g caffeine Carbon is 49.48% of the mass so you have (49.48%)*(194.19)=96.0852 g carbon to see how many carbons you have you do (mass/Molar mass) (96.0852/12.0107) = 10 So you have 10 carbons Do it for each one: Hydrogen: (5.19%)*(194.19) = 10.0785 g (mass/molar mass) (10.0785/1.00794) = 10 Nitrogen: (28.85%)(194.19) = 56.0238 g (56.0238/14.00674) = 4 Oxygen: (16.48%)(194.19) = 32.0025g (32.0025/15.9994) = 2 Final formula: C8 H10 N4 O2
Answered by sambkup - Sun Nov 1 13:44:10 2009
chemistry 101- please help?
Q. 1. Caffeine: C8H10N4O2 Consider the molecular formula for caffeine above. Using only whole numbers with no decimal point, 2 mol of caffeine has... a. ??? mol of carbon, b. ??? mol of nitrogen, c. ??? mol of hydrogen, and d. ??? mol of oxygen. 2. Consider the chemical species containing the following subatomic particles: 21 protons 23 neutrons 18 electrons a) What is the chemical symbol of the element? b) What is the mass number of this isotope?
Asked by LRumd - Wed Jan 16 18:10:44 2008 - - 2 Answers - 0 Comments
A. 1a) 16 1b) 8 1c) 20 1d) 4 (multiple the number of moles of the compound by the number of the individual atoms in the compound) 2a) 21 protons is Scandium - it's missing 2 electrons 2b) Mass number is 21+23 = 44. So Sc44
Answered by KennyB - Wed Jan 16 18:16:38 2008
Q. 1. Caffeine: C8H10N4O2 Consider the molecular formula for caffeine above. Using only whole numbers with no decimal point, 2 mol of caffeine has... a. ??? mol of carbon, b. ??? mol of nitrogen, c. ??? mol of hydrogen, and d. ??? mol of oxygen. 2. Consider the chemical species containing the following subatomic particles: 21 protons 23 neutrons 18 electrons a) What is the chemical symbol of the element? b) What is the mass number of this isotope?
Asked by LRumd - Wed Jan 16 18:10:44 2008 - - 2 Answers - 0 Comments
A. 1a) 16 1b) 8 1c) 20 1d) 4 (multiple the number of moles of the compound by the number of the individual atoms in the compound) 2a) 21 protons is Scandium - it's missing 2 electrons 2b) Mass number is 21+23 = 44. So Sc44
Answered by KennyB - Wed Jan 16 18:16:38 2008
Help on chemistry questions?
Q. There are three homework questions I'm stuck on: 1.) Caffeine is a central nervous system stimulant found in coffee, tea, and cola nuts. Calculate the molecular formula of caffeine if the compound is 49.48% C, 5.19% H, 28.85% N, and 16.48% O by mass and has a molecular weight of 194.2 grams per mole. 2.) Stannous fluoride, or "Fluoristan", is added to toothpaste to help prevent tooth decay. What is the empirical formula for stannous fluoride if the compound is 24.25% F and 75.75% Sn by mass? 3.) Calculate the number of moles of phosphorus in 14.80 grams of tetraphosphorus decaoxide, P4O10. Any help would be appreciated, but it would be great if someone could actually explain how to do these properly. I don't mind doing the work.
Asked by collegegirl23 - Sun Sep 14 22:19:52 2008 - - 1 Answers - 0 Comments
A. Moles C = 49.48 / 12.011 = 4.120 Moles H = 5.19 / 1.008 = 5.149 moles N = 28.85 g/ 14.0067 = 2.060 Moles O = 16.48 / 15.9994 = 1.030 we divide by the smallest number C4 H 5 N2 O is the empirical formula ( molar mass = 97.1) 194.2 / 97.1 = 2 molecular formula = C8H10N4O2 work in the same way
Answered by Dr.A - Mon Sep 15 10:07:04 2008
Q. There are three homework questions I'm stuck on: 1.) Caffeine is a central nervous system stimulant found in coffee, tea, and cola nuts. Calculate the molecular formula of caffeine if the compound is 49.48% C, 5.19% H, 28.85% N, and 16.48% O by mass and has a molecular weight of 194.2 grams per mole. 2.) Stannous fluoride, or "Fluoristan", is added to toothpaste to help prevent tooth decay. What is the empirical formula for stannous fluoride if the compound is 24.25% F and 75.75% Sn by mass? 3.) Calculate the number of moles of phosphorus in 14.80 grams of tetraphosphorus decaoxide, P4O10. Any help would be appreciated, but it would be great if someone could actually explain how to do these properly. I don't mind doing the work.
Asked by collegegirl23 - Sun Sep 14 22:19:52 2008 - - 1 Answers - 0 Comments
A. Moles C = 49.48 / 12.011 = 4.120 Moles H = 5.19 / 1.008 = 5.149 moles N = 28.85 g/ 14.0067 = 2.060 Moles O = 16.48 / 15.9994 = 1.030 we divide by the smallest number C4 H 5 N2 O is the empirical formula ( molar mass = 97.1) 194.2 / 97.1 = 2 molecular formula = C8H10N4O2 work in the same way
Answered by Dr.A - Mon Sep 15 10:07:04 2008
Please haelp me with these 2 questions!!!!!!!!!!?
Q. A. Determine the empirical formula for caffeine, using the following composition of a 100.00-g sample, 49.47 grams of carbon, 28.85 grams of nitrogen, 16.48 grams of oxygen, and 5.20 grams of hydrogen? B. if the molar mass of caffeine is 194.19 g/mol, calculate its molecular formula
Asked by flag - Tue Jan 19 18:04:24 2010 - - 1 Answers - 0 Comments
Q. A. Determine the empirical formula for caffeine, using the following composition of a 100.00-g sample, 49.47 grams of carbon, 28.85 grams of nitrogen, 16.48 grams of oxygen, and 5.20 grams of hydrogen? B. if the molar mass of caffeine is 194.19 g/mol, calculate its molecular formula
Asked by flag - Tue Jan 19 18:04:24 2010 - - 1 Answers - 0 Comments
Chemistry Question, Please Help!?
Q. Caffeine, a stimulant found in coffee and tea, contains 49.5% carbon, 5.15% hydrogen, 28.9% nitrogen and 16.5% oxygen by mass. What is the empirical formula of caffeine? If its molar mass is about 195g, what is its molecular formula?
Asked by unknown - Tue Sep 22 17:45:19 2009 - - 1 Answers - 0 Comments
A. Moles C = 49.5 / 12.011 = 4.12 moles H = 5.15 / 1.008= 5.11 moles N = 28.9 / 14.0067 =2.06 Moles O = 16.5 / 15.9994 = 1.03 divide by the smallest number C 4 H 5 N2 O ( empirical formula = MM = 97 g/mol) 195 / 97 = 2 multiply by 2 C8 H 10 N4 O2 is the molecular formula
Answered by Andrea - Tue Sep 22 21:50:45 2009
Q. Caffeine, a stimulant found in coffee and tea, contains 49.5% carbon, 5.15% hydrogen, 28.9% nitrogen and 16.5% oxygen by mass. What is the empirical formula of caffeine? If its molar mass is about 195g, what is its molecular formula?
Asked by unknown - Tue Sep 22 17:45:19 2009 - - 1 Answers - 0 Comments
A. Moles C = 49.5 / 12.011 = 4.12 moles H = 5.15 / 1.008= 5.11 moles N = 28.9 / 14.0067 =2.06 Moles O = 16.5 / 15.9994 = 1.03 divide by the smallest number C 4 H 5 N2 O ( empirical formula = MM = 97 g/mol) 195 / 97 = 2 multiply by 2 C8 H 10 N4 O2 is the molecular formula
Answered by Andrea - Tue Sep 22 21:50:45 2009
Determine the empirical and molecular formulas of each of the following substances.?
Q. Determine the empirical and molecular formulas of each of the following substances. A) Caffeine, a stimulant found in coffee, contains 49.5% C, 5.15% H, 28.9% N, and 16.5% O by mass and has a molar mass of 195g/mole. B) Monosodium glutamate (MSG), a flavor enhancer in certain foods, contains 35.51% C, 4.77% H, 37.85% O, 8.29% N, and 13.60% Na, and has a molar mass of 169g/mole . Please work it out so I will be able to know what to do! Thanks.
Asked by Big Dan - Tue Sep 22 14:55:51 2009 - - 2 Answers - 0 Comments
A. in 100 g of compound we have Carbon49.5g or4.125moles we also have 5.15g of hydrogen or 5.15moles of hydrogen there is 28.9g of nitrogen or 2.064285714moles of nitrogen for oxygen we have 16.5g or 1.03125moles of Oxygen in summary we have C4.125 H5.15 N2.064285714 O1.03125 dividing by the smallest we get C4 H4.99 N2.00 O1.00 the ratio is C:H:N:O=4:5:2:1 so empirical formula is C4H5N2O Empirical FW = 97 molecular weight is 195 or 2 * empirical FW molecular formula is C8H10N4O2 ~~~ in 100 g of compound we have 35.51gof carbon or 2.95916667molesof carbon we also have 4.77g of hydrogen or 4.77moles of hydrogenthe is 37.85g of oxygen or 2.365625moles of oxygento finish there is8.29g of Nitrogen or 0.592142857moles and 13.6g of… [cont.]
Answered by peter rabbit - Tue Sep 22 15:26:27 2009
Q. Determine the empirical and molecular formulas of each of the following substances. A) Caffeine, a stimulant found in coffee, contains 49.5% C, 5.15% H, 28.9% N, and 16.5% O by mass and has a molar mass of 195g/mole. B) Monosodium glutamate (MSG), a flavor enhancer in certain foods, contains 35.51% C, 4.77% H, 37.85% O, 8.29% N, and 13.60% Na, and has a molar mass of 169g/mole . Please work it out so I will be able to know what to do! Thanks.
Asked by Big Dan - Tue Sep 22 14:55:51 2009 - - 2 Answers - 0 Comments
A. in 100 g of compound we have Carbon49.5g or4.125moles we also have 5.15g of hydrogen or 5.15moles of hydrogen there is 28.9g of nitrogen or 2.064285714moles of nitrogen for oxygen we have 16.5g or 1.03125moles of Oxygen in summary we have C4.125 H5.15 N2.064285714 O1.03125 dividing by the smallest we get C4 H4.99 N2.00 O1.00 the ratio is C:H:N:O=4:5:2:1 so empirical formula is C4H5N2O Empirical FW = 97 molecular weight is 195 or 2 * empirical FW molecular formula is C8H10N4O2 ~~~ in 100 g of compound we have 35.51gof carbon or 2.95916667molesof carbon we also have 4.77g of hydrogen or 4.77moles of hydrogenthe is 37.85g of oxygen or 2.365625moles of oxygento finish there is8.29g of Nitrogen or 0.592142857moles and 13.6g of… [cont.]
Answered by peter rabbit - Tue Sep 22 15:26:27 2009
Chemistry help..please?
Q. Current Score: 0/33 Due: Friday, September 25, 2009 05:00 pm cdt view Last Response View Saved Work About this Assignment An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass 205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass 207.9766 amu. Calculate the average atomic mass. 1 amu Identify the element (Give the symbol). 2 2. 0/2 points All Submissions Notes Question: ZumChem8 3.E.042. Question part Points Submissions 1 2 0/1 0/1 5/50 0/50 Total 0/2 What number of Fe atoms and what amount (moles) of Fe atoms are in 450.0 g of iron? 1 atoms 2 moles 3. /3 points Notes Question: ZumChem8 3.E.047. Question part… [cont.]
Asked by ThatGuy88 - Thu Sep 24 02:11:13 2009 - - 1 Answers - 0 Comments
A. I wish i had assignments like this, so easy...
Answered by AJ - Thu Sep 24 02:49:49 2009
Q. Current Score: 0/33 Due: Friday, September 25, 2009 05:00 pm cdt view Last Response View Saved Work About this Assignment An element consists of 1.40% of an isotope with mass 203.973 amu, 24.10% of an isotope with mass 205.9745 amu, 22.10% of an isotope with mass 206.9759 amu, and 52.40% of an isotope with mass 207.9766 amu. Calculate the average atomic mass. 1 amu Identify the element (Give the symbol). 2 2. 0/2 points All Submissions Notes Question: ZumChem8 3.E.042. Question part Points Submissions 1 2 0/1 0/1 5/50 0/50 Total 0/2 What number of Fe atoms and what amount (moles) of Fe atoms are in 450.0 g of iron? 1 atoms 2 moles 3. /3 points Notes Question: ZumChem8 3.E.047. Question part… [cont.]
Asked by ThatGuy88 - Thu Sep 24 02:11:13 2009 - - 1 Answers - 0 Comments
A. I wish i had assignments like this, so easy...
Answered by AJ - Thu Sep 24 02:49:49 2009
Can someone help me?
Q. Problem 1 The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C6H10OS2, (a) What is the molar mass of allicin? (b) How many moles of allicin are present in 5.00 mg of this substance? (c) How many molecules of allicin are in 5.00 mg of this substance? (d) How many S atoms are present in 5.00 mg of allicin? 3.29 (a) What is the mass, in grams, of 2.50 10-3 mol of aluminum sulfate? (b) How many moles of chloride ions are in 0.0750 g of aluminum chloride? (c) What is the mass, in grams of 7.70 1020 molecules of caffeine C8H10N4O2? (d) What is the molar mass of cholesterol if 0.00105 mol weighs weighs 0.406 g?
Asked by unknown - Sat Sep 1 00:54:39 2007 - - 1 Answers - 0 Comments
A. Problem 1 (a) 6(12)+10+16+32+32 = 162 (b) 5.00mg = 0.005g Number of Moles of Allicin = 0.005/162 = 3.0864 x 10-5 (c) No. of molecules = moles x (6.02 x 10^23) = 1.86 x 10^19 (d) No. of S atoms = 1.86 x 10^19 x 2 = 3.72 x 10^19 3.29 (a) Molecular formula for Aluminium Sulfate is Al2(SO4)3 Mass of Aluminium Sulphate = Moles x RMM = 0.855g (b) Molecular formula for Aluminium Chloride is AlCl3 Moles of Aluminium Chloride = Mass/RMM = 0.0750g/RMM = 0.000561797 Moles of Cl ions = 0.000561797 x 3 = 1.69 x 10-3 (c) No. of moles = (7.70 x 10^20) / (6.02x10^23) = 0.001279069 Mass = Moles x RMM = 0.001279069 x 194 = 0.248g (d) RMM of cholesterol = mass/moles = 0.406/0.00105 = 387 (3sf)
Answered by vincentwjk - Sat Sep 1 01:22:18 2007
Q. Problem 1 The molecular formula of allicin, the compound responsible for the characteristic smell of garlic, is C6H10OS2, (a) What is the molar mass of allicin? (b) How many moles of allicin are present in 5.00 mg of this substance? (c) How many molecules of allicin are in 5.00 mg of this substance? (d) How many S atoms are present in 5.00 mg of allicin? 3.29 (a) What is the mass, in grams, of 2.50 10-3 mol of aluminum sulfate? (b) How many moles of chloride ions are in 0.0750 g of aluminum chloride? (c) What is the mass, in grams of 7.70 1020 molecules of caffeine C8H10N4O2? (d) What is the molar mass of cholesterol if 0.00105 mol weighs weighs 0.406 g?
Asked by unknown - Sat Sep 1 00:54:39 2007 - - 1 Answers - 0 Comments
A. Problem 1 (a) 6(12)+10+16+32+32 = 162 (b) 5.00mg = 0.005g Number of Moles of Allicin = 0.005/162 = 3.0864 x 10-5 (c) No. of molecules = moles x (6.02 x 10^23) = 1.86 x 10^19 (d) No. of S atoms = 1.86 x 10^19 x 2 = 3.72 x 10^19 3.29 (a) Molecular formula for Aluminium Sulfate is Al2(SO4)3 Mass of Aluminium Sulphate = Moles x RMM = 0.855g (b) Molecular formula for Aluminium Chloride is AlCl3 Moles of Aluminium Chloride = Mass/RMM = 0.0750g/RMM = 0.000561797 Moles of Cl ions = 0.000561797 x 3 = 1.69 x 10-3 (c) No. of moles = (7.70 x 10^20) / (6.02x10^23) = 0.001279069 Mass = Moles x RMM = 0.001279069 x 194 = 0.248g (d) RMM of cholesterol = mass/moles = 0.406/0.00105 = 387 (3sf)
Answered by vincentwjk - Sat Sep 1 01:22:18 2007
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