haemoglobin contains 4% iron.calculate the minimum molecular weight of haemoglobin.?
612593
let the molecular mass of haemoglobin be 'x' and let us consider 1 molecule of it.\ngiven that 4% of x = 56 (atomic mass of iron)\nthis implies x=56 * 100/4 = 56 * 25 = 1400 atomic mass units (amu)\n\nmessage to the next answerer (chemmie) - i was only following the information given in the question.. but i think you are right,, i think haemoglobin has 0.4 % Fe and not 4%... but i had to answer the question according to given data :)
844758
Using the Michaelis-Menten equation.\n\nMore details on teh attached link\n\nhttp://www.le.ac.uk/by/teach/biochemweb/tutorials/michment2print.html\n\nGood luck
389126
You don't have to 'get' equivalent weights of substances, its very simple to calculate them.\n\nFirst of all, you need to calculate the molecular wt or know the atomic wt of the compound or element you're dealing with.\n\nThe general formula for the equivalent wt of a compound is \n\nEquivalent weight = Atomic or molecular wt/ x\n\nx has different definitions in different contexts:\n\nIf for an element, x is the valency\n\nEg- E.W. of magnesium = 24/2 = 12\n\nIf for an ion, x is the number of units of charge\n\nEg- E.W. of Al+3 ion = 27/3 = 9\n\nIf for a compund, x is the total amount of formal charge present on the cation/anion, i.e. the number of ions multiplied by the charge on each radical.\n\nEg- For NaCl, the value of x would be 1\n    For MgSO4, the value of x would be 2\n    For AlCl3, the value of x would be 3\n    For Ba3(PO4)2, it would be 6,...\n\nIf for an acid, x is the basicity(no. of ionizable H+ ions)\n\nEg - 1 for HCl, 2 for H2SO4,..\n\nThe same applies for a base, x is the no. of ionizable OH- ions.\n\nNow for KMnO4 (acidified or not),\n\nThe molecular wt is 39+55+64 = 158\n\nThe value of x is 1\nSo the E.W. is 158/1 = 158\n\nHowever, if you are interested in the E.W. of Mn in KMnO4, which is more relevant in redox reactions(using acidified KMnO4), calculate the oxidation state of Mn first. It comes out to be +7.\n\nSo the E.W. is 55/7
407734
Hummm:  You can calculate the [OH-] from the pH.  [OH-] = 10^-2.  pH + pOH = 14 (from [H+]x[OH-] = 10^(-14):  pOH = 14 - 12 = 2.  Find the solubility product for iron (III) hydroxide in a table in the back of your textbook or a handbook of Chemistry or physics. Kp = [Fe+3] x [OH-]^3. Substitute numbers in and solve for [Fe+3].  This is also the molar solubility as one mole of iron hydroxide contains one mole of Fe+3.
844407
Easy, the molecular weight of HCl is 36.461 gr per mole. \n\nIf your trying to reach 4 molar solution then you need 4 x 36.461g HCL diluted to 1 liter. you need 145.844g HCl in the liter\n\nBut since your probably using 32-38 % HCl (actual amount might be on the bottle) you need to multiply you'll need to adjust for inactives by assuming your active molar mass is ~35% of 36.461 or 12.761g \n\nin order to make 1 liter of 4 molar solution you'll need 416.71g \n\n36.461/12.761 * 145.844 = 416.71\n\nassuming it is 35 % active. \n\nYou should always standardize your solution after mixing to determine final activity!!!!!
908510
It should be Fe2+ + 2OH- --> Fe(OH)2 since you not only need to balance the elements but you also need to balance the charges.
255396
FeCl3 is the limited reactant and the mass of the excess \nreactant present in the vessel is .55g Mg
975244
From the chemical equation,\n1 mole of Fe needs 2 moles of HCl for complete reaction.\nHence with 3.5 moles of Fe, you need (3.5 x 2) = 7 moles of Fe\n\nJust try ratio and proportion.\nHope this helps. :)
1125539
343.2 g of Fe2O3 - take the molar mass of Fe2O3. 2 irons is 55.85 * 2 = 111.70 grams per mole. 3 oxygens is 16 * 3 = 48. Divide 343.2 g by 159.70 g/mol and you get 2.15 moles.\n\nYour original reaction uses 2 moles of ferric oxide, so you need to multiply everything by (2.15 / 2) to get your ferric oxide to say 2.15 moles. When you do this, you will change your Kcal value to the right number.\n\n2 Fe2O3 (s) + 196.5 Kcal --> 4 Fe(s) + 3 O2 (g)\n2.15 Fe2O3 (s) + 211.2 Kcal --> 4.30 Fe(s) + 3.23 O2 (g)\n\nNote that I really didn't care about significant figures, so you should probably make sure I didn't round off incorrectly. The 2 and 4 and 3 in the equation are exact (2.0000....), but the 196.5 is an inexact number.\n\nThe second equation is easier, because you already have 0.393 in moles. You need to multiply by something that turns a 2 C3H6O into 0.393 C3H6O. So that's simply (0.393 / 2).\n2 C3H6O + 8 O2(g) --> 6 CO2 (g) + 6 H2O(g) + 853.6 kcal \n0.393 C3H6O + 1.572 O2(g) --> 1.179 CO2 (g) + 1.179 H2O(g) + 167.7324 kcal\n\nSo basically, you need to find some known number of moles, and multiply and divide your balanced equation until it has that number of moles in the equation. Then you read off whatever you need.
588190
Iron is necessary to make hemoglobin, the substance that carries oxygen through your blood to all the cells in your body. Hemoglobin is what makes red blood cells red. With insufficient iron, and therefore not enough hemoglobin, red blood cells become small and pale and don't carry enough oxygen. You may have heard the phrase "tired blood." This really means blood that is low in iron and that can't carry enough oxygen to vital organs and muscles. "Tired blood" results in a tired body. \n\nIron is needed not only for blood, but also for brains. Neurotransmitters, the neurochemicals that carry messages from one nerve to another, require sufficient iron to function properly. A person with an iron deficiency may have a tired mind as well as a tired body.
918374
Fe2O3 -- Fe+O2\n\nthis is the balanced form\n\n2(Fe2O3)--- 4Fe+3O2\nwithout the parentheses
912515
Since 56 is the atomic mass of iron then the amount here is 68.7/56 moles or 1.23 moles.\nSince 1 mole of copper is 64 g then to have 1.23 moles you need 64 X 1.23 or 78.5 g.\nThe trick is that equal numbers of moles have equal numbers of atoms.
23536
is your balace wrong?\nI only figure below balance:\nMnO2+4HCl = MnCl4+2H2O
878226
The method is very simple.  I can do the first and you can try the others.\n\n1.  First write the reaction and balance it.\n\n2HgO ---> 2Hg + O2.\n\n2. Convert grams to moles of whatever mass you have.  In this case you have O2 as 96 grams.  You convert to moles by dividing the mass by the molecular weight.  In this case, for O2 will be 32 g/mol\n\n96 grams / 32 g/mol = 3 mol.\n\n3. Now you look back to the equation.  In the equation for producing 1 mol O2 you need 2 moles of HgO.  If now have 3 moles O2, then you will need 2 x 3 moles of HgO, 6 moles.\n\n4. Now you need to convert the moles of HgO to grams.  To do this calculate the molecular weight of HgO.  It is 216.6 g/mol\n\n6 moles * 216.6 g/mol = 1299.6 g of HgO.
157730
I think FePO4 +O2 >>>>> Fe2O3 + PO2. balance it and solve it . n its simple stoichiometry.
969783
1) determine the mass of carbon, hydrogen and oxygen.\ncarbon: 6.406 g x (12 / 44) = 1.747 g\nhydrogen: 5.244 g x (2 / 18) = 0.583 g\noxygen: 4.664 - 1.747 - .583 = 2.334 g\n\n2) convert to moles.\ncarbon: 1.747 / 12 = 0.146 mol\nhydrogen: 0.583 / 1 = 0.583 mol\noxygen: 2.334 / 16 = 0.146 mol\n\n3) divide each molar amount by the lowest value\ncarbon: 0.146 / 0.146 = 1\nhydrogen: 0.583 / 0.146 = 4\noxygen: 0.146 / 0.146 = 1\n\nWe have now arrived at the answer: the empirical formula of the substance is CH4O.\nThe atomic masses add up to 32, which is also the molar mass of the compound.
47119
One gram of Fe = .450 mole\n\nMultiply that by Avogadro's number :\n0.450 mol x 6.022E -1023 \nWill yield the number of atoms in ONE GRAM...\nMultiply that number by your desired number of grams will give you your answer...