what is the formula for iron phosphate?
112589
If you are talking of iron(III) phosphate, then it should be FePO4. For iron(II) phosphate, it should be Fe3(PO4)2. Both are possible but iron(III) phosphate is more thermodynamically stable.
784111
Atomic mass of iron is 55.845 g/mol.  Get a periodic chart. The answer is there.
823190
This is a stoichiometric problem.  \n\nFirst, find the the amount in grams of one mole of Fe2O3.\n\nFor the first problem, convert the 3.02g Fe2O3 to moles.\n\nThen set up dimensional analysis.  For every 2 mol of Fe2O3, you need 2 mol C.  So you need an equal amount of moles for both.\n\nTake the amount of moles you have of Fe2O3 and convert them to grams Carbon.  \n\nFor the second problem, you should do the exact same thing except you dont need to convert to moles in the beginning because it's already in moles!\n\ni hope this is helpful!!!
977474
Ca+2 combines with PO4-3in the formula Ca3(PO4)2, calcium biphosphate\n\nCaHPO4 is another compound you may be referring to. Calcium hydrogen phosphate or calcium biphosphate
758495
The balanced equation for this reaction is :\n4Fe + 3O2 --->  2Fe2O3\nOnce you have the balanced equation, you can solve for the limiting reactant.\n0.45 mol Fe * (2 mol Fe2O3/4 mol Fe) ^^this is the mole ratio, derived from the balanced equation^^  =  .225 mol Fe2O3\nNow you have to do the same exact thing with 0.30 mole O2, your other reactant:\n0.30 mol O2 * (2 mol Fe2O3/3 mol O2) ^^once again derived from the balanced equation^^  = 0.20 mol Fe2O3\nThe limiting reactant in this reaction is O2 because it produces less moles of Fe2O3 than the Fe.\nYou use the Fe2O3 moles produced by the limiting reactant because that is all that can be produced with the "limiting" amount of reactants.  In other words, the answer is 0.20 moles of Fe2O3 are produced from the reaction.\n\nHope I helped..
599313
Refer to the electrohemical series (see source).  The answer depends on whether the conditions are such that iron is oxidized to Fe2+ or Fe3+.  In the case of iron metal being oxidized to Fe2+, the correct order is:\n\nMg, Zn, Fe, Sn, Pb
183200
It is very obvious that the answer is Fe(CO2)2 or (OOCCOO)Fe.
603812
The H's are +1, and the O's are -2, and the whole thing is 0, so...\n4(+1) + 2x + 7(-2) = 0\nx=5, so the oxidation number of phosphorus is +5.
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. :)
780875
a)4 Fe + 3O2--->2 Fe2O3\n\nCH4 + 2O2 ---> CO2 +2 H2O
465870
Iron from the hemoglobin
729557
_NaOH(aq) + _Fe(ClO4)3(aq) => _Fe(OH)3(s) + _NaClO4(aq)\n\n3  NaOH(aq) + 1  Fe(ClO4)3(aq) => 1  Fe(OH)3(s) + 3  NaClO4(aq)\nThe coefficients of one could be excluded but I put one which is also equivalent.\n\n_((NH4)2)SO4(aq) + _Pb(NO3)2(aq) => _PbSO4(s) + _NH4NO3(aq)\n\n1  ((NH4)2)SO4(aq) + 1  Pb(NO3)2(aq) => 1  PbSO4(s) + 2  NH4NO3(aq)\n\nThese are only the balanced equations.\n\nThe following is the ionic equations:\n(Na)+ (aq) + (OH)- (aq) + (Fe)3+ (aq) + (ClO4)- (aq) => Fe(OH)3(s) + (Na)+ (aq) + (ClO4)- (aq)\nand\n(NH4)+ (aq) + (SO4)2- (aq) + (Pb)2+ (aq) + (NO3)- (aq) => PbSO4(s) + (NH4)+ (aq) + (NO3)- (aq)\n\nThe ionic equations are already balanced.  It is simply the breaking down of the equations into ions.  The solid remains intact while the compounds in aqueous solution become ions.\n\nThe + and - signs are the charge of the ions.  I can't find any other way to write them so I separated the compound with parentheses.  Sorry if it's confusing.\n\nThe net ionic equations are "simplified" ionic equations.  Basically, the things that are repeated on both sides get crossed off.  What is remaining is simply the net ionic equation.\n\n(OH)- (aq) + (Fe)3+ (aq) => Fe(OH)3(s)\nand\n(SO4)2- (aq) + (Pb)2+ (aq) => PbSO4(s)
844446
AsF3=Arsenic tri fluoride\nAg2CO3=silver carbonate\nFeSO4=Iron[II] Sulfate\nP5O10=Phosphorus Di oxide or penta phosphorus deca oxide\nPb(OH)4=Lead Hydroxide
612107
a. 2k+ = .20moles , SO42-=.10moles\n\nb.Fe3+=.10moles,3NO3-= .30moles\n\nc.2Al3+=.20moles,3SO42-=.30moles\n\nd. Ni2+=.10moles,SO42-=.10moles
83000
The net ionic equation is:\n\nFe(s) + Cu2+(aq) --> Fe2+(aq) + Cu(s)
781203
2H3PO4(aq) + 3Mn(OH)2(s)  --> Mn3(PO4)2(s) + 6H2O(l)
47432
3AgC2H3O2 + Na3PO4 -----> Ag3PO4 + 3NaC2H3O2