2Fe + 3S >> Fe2S3
48.0 grams S (1 mole S/32.07 g)(2 Fe/3 mole S)(55.85 g/1 mole Fe)
= 55 .7 grams of iron needed
55,73 g of iron
ferric indicates the iron is +3 as opposed to +2 for ferrous sulfide indicates that there is sulfur with a -2 charge the formula is Fe2S3 two iron ions with a +3 = +6 3 sulfur ions with a -2 = -6 -6+6 = 0
These are the ions and their charges: Fe+3 SO3-2The charges have to add up to zero, so two +3 iron ions cancel out three -2 sulfite:Fe+3 Fe+3 SO3-2 SO3-2 SO3-2Simplify: Fe2(SO3)3
If you're talking about Iron (II) Sulfide, where the oxidation of Iron is 2+, 2 electrons from the Iron atom is transferred to the Sulfur atom, producing Fe2+ and S2- .
The chemical formula is... Fe2S3
55,73 g of iron
When heat is applied to the mixture of metal fillings and sulfur, a chemical reaction occurs. The heat provides the energy necessary for the atoms of the metal and sulfur to rearrange and form new chemical bonds, resulting in the formation of a new substance with different properties than the original components. This process is called a chemical change, where the original substances react to form different compounds.
The balanced chemical reaction for the formation of iron(II) sulfate from metallic iron and solid sulfur is: 3 Fe(s) + 3 S(s) → Fe2(SO4)3(s)
decomposition
The chemical formula for ironite trisulfide is Fe2S3. It consists of two iron (Fe) atoms and three sulfur (S) atoms.
.2M x V FeCl3=moles FeCl3 x 1mole Fe2S3/2mole FeCl3=moles of Fe2S3 x mm of Fe2S3/1 mole Fe2S3= g Fe2S3 x .65% yield. 2.75g Fe2S3/ .65= 4.23g Fe2S3/ 207.91= .02035 x 2mole FeCl3=.0407 moles FeCl3/ .2M FeCl3= .2035 L x 1000= 203.5 ml
ferric indicates the iron is +3 as opposed to +2 for ferrous sulfide indicates that there is sulfur with a -2 charge the formula is Fe2S3 two iron ions with a +3 = +6 3 sulfur ions with a -2 = -6 -6+6 = 0
Iron has a charge of +3 and Sulfur has a charge of -2, so iron III sulfide is: Fe2S3
To calculate the maximum amount of Fe2S3 that can be formed, we need to determine the limiting reactant. Using the balanced equation for the reaction between Fe and S to form Fe2S3, we find that 8 moles of S react with 3 moles of Fe. From 17 g of S, we can calculate the amount of Fe2S3 that can be formed by converting the mass of S to moles and using the mole ratio from the balanced equation.
Sulfur and iron are both elements. An element is a pure substance that cannot be broken down into simpler substances through chemical reactions. Sulfur and iron are classified as elements based on their chemical properties.
In cases of particular elements during reactions we see the change is their individual oxidation states.But if we have to calculate the equivalent weight of a species in a particular reaction,we have to find out the n factor for that particular species in the reaction.It is basically the overall exchange of electrons of a species per mole of that species in the reaction. And 1 thing more,n factor can never be calculated for individual atoms. For example:if we have to find out the equivalent weight of Fe2S3 in the reaction Fe2S3 --> FeSO4 + SO2 First v balance the equation which gives Fe2S3 + 502-->2FeSO4 +SO2 Then v find out the oxiadation states of S in d differsnt compounds cos v c that S is the only common element in all.In Fe2S3 The ox.state of s is -2.In FeS04 it's +6 n in SO2 it's +4. So we c the net exchange of electrons per mole of Fe2S3 in d reaction is 2*(+6-(-2))+(4-(-2)) = (2*8)+6 =22 Therefore the n factor of Fe2S3 is 22. So its equivalent weight will be Molecular weight/22.
Iron reacts with sulfur to form ferrous sulfide (FeS) instead of ferric sulfide (Fe2S3) because iron(II) ions (Fe2+) have a lower oxidation state compared to iron(III) ions (Fe3+). In this reaction, iron gains two electrons to form Fe2+ ions, which then combine with sulfide ions to form ferrous sulfide.