How do you predict the chemical reaction of a formula?
84780
!!!!!!!!!!!!!!!! \nI think rather u wanted to ask how can u predict the formula of a chemical reaction!!\nFirstly, we have to determine the moles of reactant taking part.(It can be done easily, think A reacts with B, just mix 1 mole of A with the same amount of B.)\nThen determine what are the different products and their amounts.\nAll u have to do is some calculations..................\nRemember its not as easy as it sounds.
846447
http://www.bbc.co.uk/schools/gcsebitesize/chemistry/classifyingmaterials/formulae_and_equationsrev4.shtml
707973
You have to start with a balanced equation.  The subscripts will give you the correct charge and a prefix will give you the right amount of atoms on each side of the equation.  Some elements, like O, F, and I are diatomic and come in pairs.
50274
Chemical equations show the molecular composition of compounds in a balaanced form between reactants and products. These are expressed in moles, or number of molecules, rather than mass. By matching the number of molecules needed for a reaction the result can be controlled better than if only mass were used. Excess or limited amounts of one element in a reaction might cause the product to be different than intended. Ultimately, a chemical engineer will convert the specifications to mass, but unless the molarity of the raw material is known this cannot be done properly.
861726
You will have to first find the standard enthalpy values of the reactants and products. They're given in the appendices of any standard GenChem or PhysChem books.\n\nThen, you subtract the sum of enthalpies of reactants from the sum of enthalpies of the product to get the enthalpy of the reaction.
856873
The balanced chemical equation and the molecular weights of the reactants and products.\n\nIn simplest form, assume\n\nXY + AB = XB + AY.\n\nAssume the molecular weight of XY is 50, and of XB 35.\n\nFor every 50 grams (or pounds, tons, or any other measure of mass) of XY you use, you will get 35 grams (or whatever) of XB.\n\nEDIT:\n\nOK. Atomic weights are H=1, S=32, Cl=35.5, Fe=56. Molecular weights are FeS=88, HCl=36.5, H2S=34, FeCl2=127.One gram molecular weight of each is its molecular weight in grams. So if you react 88 grams of FeS with 36.5 x 2 grams of HCl (the balanced equation tells you that you need 2 moles of HCl, so you multiply by 2), you will get 34 grams of H2S and 127 grams of FeCl2. \n\nNotice that the weights balance. You put in 88 + (36.5 X 2) grams, or 161 grams. You got out 127 + 34, or 161 grams.\n\nYou need the mass of any one of those compounds - either reactant or product - to determine all the others. Calculate the moles of the one for which you have the mass, determine the ratio of the moles of that one to the others, multiply by that ratio and then multiply result by molecular weight.
688944
View source of the that page.\nYou will see the formulas.
250561
i can help with part of it. i forgot a lot of my chemistry stuff. so ok  first thing is to find the number of mols of each reactant put in. which is  mass over molar mass. and then find the molar mass of 0.566g of H2. so you know how many moles of H2 are left over, so you should lknow how many moles reacted and you should know the number of mols of the other 2 substances too and you know the volume and you can figure out the masses so then   do that. \nand Kc is just the  conc of products over reactants. if youre in AP   i assume you know how to do that\nthen c   and    um partial pressures. i think it has something to do with mole ratios and   the total pressure. im not completely sure, but im sure you can figure it out. good job
123634
http://members.aol.com/oelaineo/formulas.html
691513
Check that both sides of equation match. Here is an example:\n\n3 CH3CH2OH + 2 Cr2O7 2- + 16 H+ --> 3 CH3COOH + 4 Cr3+ + 11 H2O\n\nThere should be an equal amount of H, C, O, Cr in both sides of the equation. \nIt is sometimes difficult to know where to start balancing an equation. In such case you should try to find an element/molecule that does not appear in every molecule on the other side of the equation. Eg. when balancing this equation above, I first balance the number of Cr because it is on its own on the right side. Sometimes you just need to try and play with numbers for a while to find the right answer. Hope this helped...
460906
DH reaction = DH products – DH reactants\n\nExample:  2A + B -- C\nDH = DH C – (2 DH A + DH B)\n\nIf DH is negative: exothermic reaction \nIf DH is positive: endothermic reaction
1117999
First make a chemical equation, balance it, and find a mole ratio.  Use that ratio and the above information to solve the problem.
264121
The theory can be used to calculate the mass of product that is expected to be produced when more than one reactant is involved in its formation.\nConsider the reaction below:\n\n2Na2S + Na2CO3 + 4SO2 ---> 3Na2S2O3 + CO2 \n\nGiven the mass of the reactants involved, we would use just one of them as a reference to get the mass of the product, but which reactant should we choose? \n\nHere we find the moles of each of the 3 reactants (given the mass)  and then compare the moles ratio of each in turn with the product and hence calculate the moles of the product Na2S2O3. A limiting reactant is one which gives the least moles of the product. So we see that from which reactant we get the least moles of Na2S2O3, and then with the moles, we can finally calculate the mass of product we expect to get when the reaction is carried out.\nWe choose the limiting reactant for finding out the yield because after any one of the reactants is used up,  the reaction won't proceed further, so this is to calculate the maximum amount of product we can get.
919460
its actually pretty simple. U multiply by -1 when u flip over an equation...so the reactants become the products and the products the reactants. that way instead of having a negative number u will have a positive number for the kJ. as in this problem. U have to flip #1 so u can cancel a few things with #2. so it becomes..\n1)3 H2O(l) + 2 CO2(g) AH---->CH3CH2OH(l) + 3 O2(g) (multiply by -1 gives u a postive +1367kJ. part two stays the same.\n2) C2H4(g) + 3 O2 ---> 2 H2O(l) + 2 CO2 (g) AH= -1411 kJ\n\nNow the 3 O2 from #1 and #2 cancel since they are on opposite sides. Now the 2 H20 cancel from #2 and you are left with only one in #1 since they are also on opposite sides...which after canceling..leaves u with your original equation.\n\nC2H4(g) + H2O(l) ------> CH3CH2OH(l)\n\nnow since u flipped over #1.....and u have a positive +1367kJ and\n#2 is left the same...its still at negative -1411kJ. u add them together and u get an enthalpy change of -44kJ. sorry its pretty confusing to explain..if anything message me and i willl try to help.
865969
Yes they react, for example:\n\nCH3COOCH2CH3 + HCOOH  <==> HCOOCH2CH3 + CH3COOH
986414
Start by balancing the equation:\n2Ca3(PO4)2 (s) + 6H2SO4 (aq)-----> 6CaSO4 (s) + 4H3PO4(aq)\n\nThen figure out the molar masses of each of the reactants:\nCa3(PO4)2 = 3(40.078) + 2(30.973762) + 8(15.9994) = 310.176724\n\nH2SO4 = 2(1.00794) + 32.065 + 4(15.9994) = 98.07848\n\nDivide each of your known masses of reactants by its respective molar mass to determine how many moles of each you have, and divide this number by the coefficient (the number in front) of the reactant to determine how many "parts" of each you have:\n(1000/310.176724)/2 = 1.612 parts 2Ca3(PO4)2\n(980/98.07848)/6 = 1.665 parts 6H2SO4\n\nTake the smaller number (since once you run out of one reactant, the reaction is over) and figure out how many moles of calcium sulfate and phosphoric acid you'll produce:\n(1.612)(6)(40.078 + 32.065 + 4(15.9994)) = 1316.7518832g CaSO4\n\n(1.612)(4)(3(1.00794) + 30.973762 + 4(15.9994)) = 631.872933536g H3PO4\n\nSince the total mass of reactants and products needs to be the same, you can check your (er, my) work by totalling up both sides:\n(1.612)(2)(310.176724) + (1.612)(6)(98.07848) = 1948.625g\n1316.7518832 + 631.872933536 = 1948.625g
761935
when in a chemical reaction