1. Convert what you have into moles. mols Fe(NH4)2(SO4)2.6H2O = g/molar mass. 1.0 M x 0.013L = mols H2C2O4.
2a. Convert moles Fe compound to moles of the product.
2b. Convert moles H2C2O4 to moles of the product.
2c. The smaller of 2a or 2b will be the limiting reagent. Pick that for the moles of the product.
3. Convert mols of product to grams of product: moles product x molar mass = grams.
Problem 2.
H2O2 + Fe(II) ==>
I would separate into the two half quations.
Fe^+2 ==> Fe^+3
H2O2 + H^+ ==> 2H2O
Balance the two half equations, multiply by appropriate numbers to make the electrons equal, add them, count the electrons changed.
problem 3. Remember the definitions.
Oxidation is the loss of electrons (and the element oxidized is the reducing agent.)
Reduction is the gain of electrons (and the element reduced is the oxidizing agent).
Post your work if you get stuck on any of these.
These are the problems I am having trouble with.
1.The first step of the synthesis is described by the reaction below. When 1.750 g of Fe(NH4)2(SO4)2 6H2O is mixed with 13 mL of 1.0 M H2C2O4 , the theoretical yield of FeC2O42H2O is
how many grams?
Fe(NH4)2(SO4)26H2O(s) + H2C2O4(aq)
FeC2O42H2O(s) + (NH4)2SO4(aq) + H2SO4(aq) + 4 H2O(l)
2.How many electrons are transferred in the reaction of hydrogen peroxide with iron (II) ion in
acidic solution to form iron (III) ion and water?
3.In the reaction of hydrogen peroxide with iron (II) ion in acidic solution to form iron (III) ion and water,
the oxidizing agent is
2 answers
what is H2C2O4
2 answers