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How many grams of iron can be made form 119 g of Fe2S3 and 12.7 g C?
To determine the amount of iron that can be produced from 119 g of Fe2S3 and 12.7 g of C, we first need to calculate the molar mass of Fe2S3 and C. The molar mass of Fe2S3 is approximately 207.9 g/mol, and the molar mass of C is approximately 12.01 g/mol. Next, we calculate the moles of Fe2S3 and C by dividing the given masses by their respective molar masses. Then, we determine the limiting reactant by comparing the moles of Fe2S3 and C. Finally, we use the stoichiometry of the balanced chemical equation to calculate the theoretical yield of iron, which is approximately 42.4 grams.
What does Fe2S3 break down into?
Iron(III) sulfide (Fe2S3) breaks down into iron(III) oxide (Fe2O3) and sulfur dioxide (SO2).
What is the symbol of iron sulphide?
FeS is Iron II Sulfide Fe2S3 is Iron III Sulfide
What is the formula for ironIII sulfide?
Fe2(SO3)2 I don't think the above answer is right...I believe it is Fe2S3
How many grams of iron can be found in a 130 g sample of iron III sulfide?
The formula of iron (III) sulfide is Fe2S3, showing that each formula unit contains two iron atoms. The gram formula unit mass for iron (III) sulfide is 207.87, and the gram atomic mass of iron is 55.847. Therefore, the fraction by mass of iron in iron (III) sulfide is 2(55.847)/207.87 or about 0.5373, and the grams of iron in 130 g of iron (III) sulfide is 0.5373 X 130 or 69.9 grams, to the justified number of significant digits.
How do you write a balanced equation for FeCl3 and Na2S)?
1. Add a small quantity of the FeCl3 solution into the Na2S(aq.). 2FeCl3+3Na2S=2FeS↓+6NaCl+S↓ the following is the ionic reaction equation 2Fe3+ + S2- = 2FeS↓+ S↓ 2. Add a small quantity of the Na2S solution into the FeCl3(aq.) 2FeCl3 + Na2S =2FeCl2 + 2NaCl + S↓ the following is the ionic reaction equation 2Fe3+ + S2- = S↓ + 2Fe2+
Chemical formula For Ironite Trisulfide?
The chemical formula for ironite trisulfide is Fe2S3. It consists of two iron (Fe) atoms and three sulfur (S) atoms.
What is the chemical formula for iron sulfate?
The chemical formula is... Fe2S3
How many grams of Fe2S3 can be formed from 17 g S and excess of Fe?
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.
Hydrogen sulfide gas is bubbled through a solution of iron III chloride what is produced?
When hydrogen sulfide gas is bubbled through a solution of iron III chloride, it forms iron III sulfide as a solid precipitate. This reaction is represented by the chemical equation: FeCl3 + 3H2S -> Fe2S3 + 6HCl.
What is the chemical formula for Fe3 combined with S2?
The chemical formula for iron (III) sulfide, which is made up of iron (Fe^3+) and sulfide ions (S^2-), is Fe2S3. It is important to note that the charges on each ion must balance in the compound to maintain charge neutrality.
How many grams of iron can be made form 119 g of Fe2S3 and 12.7 g C?
To determine the amount of iron that can be produced from 119 g of Fe2S3 and 12.7 g of C, we first need to calculate the molar mass of Fe2S3 and C. The molar mass of Fe2S3 is approximately 207.9 g/mol, and the molar mass of C is approximately 12.01 g/mol. Next, we calculate the moles of Fe2S3 and C by dividing the given masses by their respective molar masses. Then, we determine the limiting reactant by comparing the moles of Fe2S3 and C. Finally, we use the stoichiometry of the balanced chemical equation to calculate the theoretical yield of iron, which is approximately 42.4 grams.
The oxidation number of Fe in Fe2S3 is?
The oxidation number of Fe in Fe2S3 is +3. This can be determined by setting up an equation where the total oxidation number of the compound is equal to zero, and solving for the unknown oxidation number of Fe.
How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 2.75 g of Fe2S3 if the percent yield for the reaction is 65.0 percent?
.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
What is the chemical formula for ferrous disulfide?
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
How many grams of iron are contained in 34 grams of fe2s3?
To calculate the amount of iron in Fe2S3, first find the molar mass of Fe2S3: Iron (Fe) has a molar mass of 55.85 g/mol and sulfur (S) has a molar mass of 32.06 g/mol. So, the molar mass of Fe2S3 is 2(55.85) + 3(32.06) = 222.92 g/mol. Next, divide the molar mass of iron by the molar mass of Fe2S3 and multiply by the given mass of Fe2S3 to find the grams of iron: (2 * 55.85 g/mol / 222.92 g/mol) * 34 g = 8.53 g of iron in 34 g of Fe2S3.
Formula for ironIIIsulfide?
Formula: Fe2S3
