Molecular Ibuprofen Resource

Molecular Ibuprofen Posts

Questions and Answers

How does Ibuprofen act on the molecular level? That is how does ibuprofen exert its pain killing action?

jamescotton replied: "Ibuprofen is an NSAID which is believed to work through inhibition of cyclooxygenase (COX), thus inhibiting prostaglandin synthesis. There are at least 2 variants of cyclooxygenase (COX-1 and COX-2). Ibuprofen inhibits both COX-1 and COX-2. It appears that its analgesic, antipyretic, and anti-inflammatory activity are achieved principally through COX-2 inhibition; whereas COX-1 inhibition is responsible for its unwanted effects on platelet aggregation and the GI mucosa."

jessica b replied: "DRUG CLASS AND MECHANISM: Ibuprofen belongs to a class of drugs called non–steroidal anti–inflammatory drugs (NSAIDs). Other members of this class include aspirin, naproxen (Aleve), indomethacin (Indocin), nabumetone (Relafen) and several others. These drugs are used for the management of mild to moderate pain, fever, and inflammation. Pain, fever, and inflammation are promoted by the release in the body of chemicals called prostaglandins. Ibuprofen blocks the enzyme that makes prostaglandins (cyclooxygenase), resulting in lower levels of prostaglandins. As a consequence, inflammation, pain and fever are reduced. The FDA approved ibuprofen in 1974."

Determine molecular formula for the headache remedy Ibuprofen? Molar mass is 206 g/mol precent composition 75.7% C, 8.80% H, 15.5% O thanks so much im really having a rough time w/ chemistry

derrp replied: "If you assume a 100g sample of ibuprofen, it will contain: 75.7g C 8.80g H 15.5g O If you convert those masses to moles (using each element's molar mass) and use the moles as subscripts for each element, you will have a rough molecular formula. Divide all the subscripts through by the value of the smallest subscript, then multiply them all by an integer factor in order to convert them all to whole number subscripts. [C(6.303)H(8.73)O(0.96875)]/(0.96875) = C(6.506)H(9.0116)O(1) = [C(6.506)H(9.0116)O(1)]*2 = C(13.012)H(18.023)O(2) = C13H18O2 And you can check your answer with Wikipedia (source link). It's actually pretty reliable for science and math topics."

skipper replied: "Calculate the moles of C, H, and O in 100 grams: 75.7 g C / 12.011 g/mol = 6.303 mol C atoms 8.80 g H / 1.008 g/mol = 8.730 mol H atoms 15.5 g O / 16.00 g/mol = 0.969 mol O atoms Determine the ratio of O:C:H by dividing by the smallest C: 6.303 / 0.969 = 6.5 H: 8.730 / 0.969 = 9.0 O: 0.969/0.969 = 1.0 Multiply all by 2 so that you have whole numbers- C = 2x6.5 = 13 H = 2x9.0 = 18 O = 2x1 = 2 Empirical formula = C13H18O2 (molar mass = 206) Therefore the empirical formula is the molecular formula"

Ibuprofen's emprical and molecular formula...? The common pain medicine, Advil, contains the active ingrediant Ibuprofen that has a molar mass of 206 g mol -1. Ibuprofen contains 75.73% C, 8.74% H, and the remainder being oygen. What are the empircal and molecular formulas for Ibuprofen.? I really need help with this question. Would you please help me set of the question? The help with be greatly apppreciated.

milton b replied: "C13H18O2 is the molecular formula"

R S replied: "Empirical Formula: Information Given: 1 mol = 206g 75.73% C, 8.74% H Therefore, 15.53% O. First you have to understand that these percentages are in accordance to mass. (75.73% of the total mass is C...etc) So, let's assume that you have 1 gram of ibuprofen. of that 1 gram, 0.7573 g of it will be C and so on. Now that we have actual masses to work with, we can calculate the molar ratios between the different elements that comprise ibuprofen. Using dimensional analysis: 0.7573 g of C / 12.0 g/mol = 0.0631 mols of C 0.0874 g of H / 1.0 g/mol = 0.0874 mols of H 0.1553 g of O / 16.0 g/mol = 0.0097 mols of O After getting these ratios, think back and remember when your teacher talked about THE LAW OF MULTIPLE PROPORTIONS. This law states that elements combine with each other in whole numbers. In order to make these ratios whole numbers, you would divide all of them with the smallest ratio in order to reduce that smallest ratio to 1 - the smallest whole number. So: H: 0.0874 mols / 0.0097 mols = 9.00 C: 0.0631 mols / 0.0097 mols = 6.51 O: 0.0097 mols / 0.0097 mols = 1 What this tells us is that the ratio of H:C:O is 9 : 6.5 : 1 Now following the law of multiple proportions, we have to make sure that these values are whole numbers. To do this, we must multiply the ratios by 2 resulting in a: 18 : 13 : 2 ratio. Therefore your empirical formula would be: C13H18O2. Molecular Formula: Now that we have the empirical formula, which is the lowest possible ratio of the element which comprises ibuprofen, we can find the molecular formula. It is given that 1 mol of ibuprofen has a mass of 206 g. So then, how much mass would 1 g of the stuff in your empirical formula have? (13 atoms of C x 12.0 g/mol) + (18 atoms of H x 1.0 g/mol) + (2 atoms of O x 16.0 g/mol) = 206 g/mol. So coincidentally, the molar mass of your empirical formula is the same as the given 206g in 1 mole of ibuprofen. Therefore your empirical formula is the same as the actual molecular formula. ( C13H1802 ) If ibuprofen had a molar mass of 412 g/mol, then your empirical formula would be half of the molecular formula. In that case, your molecular formula would be C26H32O4. You're welcome. RS"

how does ibuprofen act on a molecular level? how does it exert its ain killing action

Andrea replied: "probably blocks the chemical reactions in your brain from reaching the place where sensations are processed."

Troy replied: "The beneficial effects come from COX II inhibition, an enzyme responsible for synthesis of cytokines that cause pain and inflammation. It is also a COX I inhibitor, which is where much of the adverse effects come from (most notably GI irritation )"

Finding empirical and molecular formulas? Determine the empirical and molecular formulas of ibuprofen composed of C, H and O. The mass percent composition of ibuprofen was found to be 75.69% C, and 8.80% H and the molecular mass of ibuprofen is 206 amu.

kodie replied: "Empirical formulas... 1. Start with the number of grams of each element, given in the problem. If percentages are given, assume that the total mass is 100 grams so that the mass of each element = the percent given. 2. Convert the mass of each element to moles using the molar mass from the periodic table. 3. Divide each mole value by the smallest number of moles calculated. 4. Round to the nearest whole number. This is the mole ratio of the elements and is represented by subscripts in the empirical formula. If the number is too far to round (x.1 ~ x.9), then multiply each solution by the same factor to get the lowest whole number multiple. e.g. If one solution is 1.5, then multiply each solution in the problem by 2 to get 3. e.g. If one solution is 1.25, then multiply each solution in the problem by 4 to get 5. Once the empirical formula is found, the molecular formula for a compound can be determined if the molar mass of the compound is known. Simply calculate the mass of the empirical formula and divide the molar mass of the compound by the mass of the empirical formula to find the ratio between the molecular formula and the empirical formula. Multiply all the atoms (subscripts) by this ratio to find the molecular formula. 1) C = 75.69% = 75.69 g H = 8.80% = 8.80g O = 100 - %C - %H O = 100 - 75.69 - 8.80 = 15.51% = 15.51g 2) n = m / M n = moles m = mass (g) M = molar mass (gmol^-1) n(C) = 75.69g / 12gmol^-1 = 6.3075 mol n(H) = 8.80g / 1gmol^-1 = 8.80 mol n(O) = 15.51g / 16gmol^-1 = 0.969375 mol 3) Divide each mole value by the smallest number of moles calculated. in this case, n(O) = 0.969375 mol C = 6.3075 mol / 0.969375 mol C = 6.506769826 H = 8.80 mol / 0.969375 mol H = 9.078014184 O = 0.969375 mol / 0.969375 mol O = 1 4) multiply each value by 2 to get whole numbers; C = 6.506769826 x 2 = 13.01353965 H = 9.078014184 x 2 = 18.15602837 O = 1 x 2 = 2 thus, empirical formula = C13H18O2 Molecular formula....... first, find the molar mass of the empirical formula M(C13H18O2) = (13 X 12) + (18 X 1) + (2 X 16) M(C13H18O2) = 206 gmol^-1 then find the ratio between the molar mass of the empirical formula and that of the molecular mass that you are given; 206/206 = 1 thus, empirical formula = molecular formula = C13H18O2 hope this helps:-)"

xener70 replied: "(Cx Hy Oz)n Taking 100g of ibuprofen: 1- calculate the moles of each atom in that amount C ---- 75.69/12 = 6.308 H ---- 8.8/1 = 8.8 O ---- 15.51/16 = 0.9694 2- evaluate the relation of atoms in the moleucule. dividing each moles of elements by the lowest value above. C ---- 6.308/0.9694 = 6.5 H ---- 8.8/ 0.9694 = 9 O ---- 1 As the molecule has only "natural number" amounts of atoms: multiply the values by two (C13 H18 O2) n and this is the empiric formulae in order to know the molecular formula we compare the weight of the empiric formulae to the real value. (13*12 + 18*1 + 16*2)*n = 206 this means that n=1, so the molecular formula is C13 H18 O2"

Chemical and Empirical formula of Ibuprofen? Ibuprofen, a headache remedy, contains 75.69% C, 8.80%H, 15.51% O by mass, and has a molar mass of 206g/mol. what is the empirical and molecular formula of Ibuprofen?

ASB08 replied: "This is what is called a compositional stoichiometry problem. First, let's imagine that you have 100 g of ibuprofen. If you imagine this, then you realize that you have the gram equivalents of the percentage, so 75.69 g C, 8.80 g H, and 15.51 g O. Convert each of these masses to moles using their molar masses. When you have the number of mols of each, divide each amount of mols by the smallest number available. For example, if you end up with 6.3 mol C, 8.8 mol H, and 1 mol O, then you would divide each number by 1 because it is the smallest. If your answers to the previous step come out to whole numbers or VERY CLOSE to whole numbers, then you can stop. That's your empirical formula! If not... then multiply all numbers by an integer until this happens and you will get your empirical formula. Next, find the ratio of the empirical mass to the molecular mass. The molecular mass is 206 g, so if the empirical mass is also 206 g, then you have your molecular formula too! If the empirical mass is 1/3 of the molecular mass, multiply your emiprical formula by 3 to attain your molecular mass (Recip. of ratio). It is very important that you keep many decimal places in this whole process until the very last step, which is writing the empirical and molecular formulas. If you don't, then your answer will be off! Hope this helped..."

hawkeye3772 replied: "So, 100g of ibuprofen would contain 75.69g C, 8.80g H, and 15.51g O. 75.69/12.01 = 6.302 mol C 8.80/1.01 = 8.713 mol H 15.51/16 = .969 mol O now divide by the smallest number 6.302/.969 = 6.5 C 8.713/.969 = 9.0 H .969/.969 = 1.0 O multiply everything by 2 to get all whole numbers 6.5 x 2 = 13 C 9.0 x 2 = 18 H 1.0 x 2 = 2 O so the empirical formula is C13H18O2 C13H18O2 = 206g/mol the molecular formula is also C13H18O2"

molecular formulas......? I know that say the molecular formula of ibuprofen is C13H18O2 But why does it go carbon atoms, then hyrogen then oxygen? Why in that specifc order? Could it be H18O2C13??? Does it ALWAYS go carbon atoms, then hydrogen, then oxygen?

Jen S replied: "In general, if a molecule contains Carbon, those are listed first, second is hydrogen, third is oxygen, and then in general other atoms are listed in order of their electronegativities."

Mardy Bum replied: "It has to deal with the way they're bonded and their actual structure. You never see carbon atoms bonded to hydrogen, but rather hydrogen attached to carbon. Except in the case of water, where it's structure is actually HOH."

MrCool56 replied: "Perhaps it is just tradition or maybe it is from the IUPAC - International Union of Pure and Applied Chemistry. Which governs the nomenclature of chemicals. If everyone writes with the same formulae and chemical names in the same way then there will be no confusion. "

Doc89891 replied: "No particular reason - its customary. However the CHO listing does tell you quickly that you are dealing with a hydrocarbon. People are used to doing it that way is what it amounts to."

help with the molecule ibuprofen?? does anybody know the lewis structure of ibuprofen? or a list of the inter molecular forces it contains?

lucky_ducky331 replied: "http://www-home.cr.duq.edu/~harrold/Chem3D/ibuprofen.JPG and look up Ibuprofen on."

More Websites

Molecular Expressions: The Pharmaceutical Collection - Ibuprofen
Ibuprofen is a nonsteroidal anti-inflammatory drug that is used to treat symptoms caused by arthritis, such as swelling, pain, and stiffness.

Ibuprofen's emprical and molecular formula...? The common ...
Empirical Formula: Information Given: 1 mol = 206g 75.73% C, 8.74% H Therefore, 15.53% O. First you have to understand ... which comprises ibuprofen, we can ...

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Ibuprofen - PubChem Public Chemical Database
PubChem ... Ibuprofen is a white powder with a melting point of 74-77C and ... Molecular Mechanisms of Pharmacological Action. Enzyme Inhibitors ...

CAS No.15687-27-1,Ibuprofen Suppliers,MSDS download
LookChem is the world's leading B2B trading platform for chemicals. ... Molecular Structure: Name:Ibuprofen. CAS Number:15687-27-1. Molecular Formula:C13H18O2 ...

CAS No.51146-56-6,S-(+)-Ibuprofen Suppliers
LookChem is the world's leading B2B trading platform for chemicals. ... Molecular Structure: Name:S-(+)-Ibuprofen. CAS Number:51146-56-6. Molecular Formula:C13H18O2 ...

Ibuprofen Manufacturer, Buyer, Supplier, Importer, Exporter ...
Trade Leads for ibuprofen, Search ecplaza.net for buying and selling leads, ... Ibuprofen Molecular formula : C13H18O2 MW : 206.27 CAS No. :15687-27-1 Assay:99 ...

Ibuprofen Oral Suspension Official FDA information, side ...
Accurate, FDA approved Ibuprofen Oral Suspension information for healthcare ... The molecular weight of ibuprofen is 206.28. Its molecular formula is C13H18O2 ...

Ibuprofen - wikidoc
Pharmacokinetics and Molecular Data. FDA label. FDA on Ibuprofen. Return to top ... Articles on Ibuprofen in N Eng J Med, Lancet, BMJ. WikiDoc State of the Art Review ...

Insights from molecular dynamics simulations into pH ...
... on the hydrolysis of ibuprofen esters by Candida rugosa lipase ... Models, Molecular. Substrate Specificity. Substances: Amino Acids. Ibuprofen. Lipase ...