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

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.

what is H2C2O4

To solve these problems, we will analyze each question step-by-step:

1. Calculation of Theoretical Yield:
Theoretical yield refers to the maximum amount of product that can be obtained in a chemical reaction. In this case, we are given the mass of starting material (Fe(NH4)2(SO4)2 6H2O) and the volume and concentration of the reactant (H2C2O4). To find the theoretical yield of FeC2O42H2O, follow these steps:
- Calculate the number of moles of Fe(NH4)2(SO4)2 6H2O by dividing the given mass by its molar mass.
- Use the balanced chemical equation to determine the mole ratio between Fe(NH4)2(SO4)2 6H2O and FeC2O42H2O.
- Convert the moles of Fe(NH4)2(SO4)2 6H2O to moles of FeC2O42H2O using the mole ratio.
- Convert the moles of FeC2O42H2O to grams using its molar mass.

2. Calculation of Electrons Transferred:
In the given reaction of hydrogen peroxide (H2O2) with iron (II) ion (Fe2+) to form iron (III) ion (Fe3+) and water (H2O), we need to determine the number of electrons transferred. Follow these steps:
- Identify the oxidation states of each element involved in the reaction.
- Notice the change in oxidation states for the elements undergoing oxidation and reduction.
- Determine the difference in the number of electrons lost and gained.
- Make the necessary adjustments to balance the half-reactions if required.

3. Identification of the Oxidizing Agent:
In the reaction of hydrogen peroxide (H2O2) with iron (II) ion (Fe2+) to form iron (III) ion (Fe3+) and water (H2O), we need to identify the oxidizing agent. The oxidizing agent is the species causing oxidation by accepting electrons from another substance. Follow these steps:
- Determine the oxidation states of each element involved in the reaction.
- Notice which element undergoes an increase in its oxidation state.
- The species causing the increase in oxidation state is the oxidizing agent.