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Is Fe2S3 molecular or ionic compound?
Fe2S3 is an ionic compound. It is composed of iron (Fe) cations and sulfide (S) anions, which form an ionic bond through the transfer of electrons.
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.
What is the correct name for the compound Fe2S3?
Ferrous Sulfide = Iron (III) Sulfide Both -> 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.
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.
Is Fe2S3 molecular or ionic compound?
Fe2S3 is an ionic compound. It is composed of iron (Fe) cations and sulfide (S) anions, which form an ionic bond through the transfer of electrons.
What type of reaction is Fe2S3 equals 2Fe plus 3S?
decomposition
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
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
What does Fe2S3 break down into?
Iron(III) sulfide (Fe2S3) breaks down into iron(III) oxide (Fe2O3) and sulfur dioxide (SO2).
In which type of bond are electrons?
Electrons are shared in a type of bond known as covalent. This type of bond is also considered a chemical bond.
2 Fe + 3 S -> Fe2S3?
Fesub2 S
What is the correct name for the compound Fe2S3?
Ferrous Sulfide = Iron (III) Sulfide Both -> 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.
How many grams of iron can be made form 119 g of Fe2S3 and 12.7 g C?
To find how many grams of iron can be produced, calculate the molar mass of Fe2S3 and C, then use stoichiometry to determine the amount of Fe that can be produced. 1 mole of Fe2S3 produces 2 moles of Fe, and 1 mole of C produces 3 moles of Fe, so compare the moles of Fe produced from each reactant and choose the limiting reactant. Calculate the amount of Fe produced.
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.
