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In the reaction 2 Fe plus 3 S--- Fe2S3 how much iron is required to react with 48.0 g of sulfur?
To determine the amount of iron required, you first need to find the molar mass of sulfur (32.06 g/mol) and the molar mass of iron (55.85 g/mol). Then, use the stoichiometry of the reaction to calculate the amount of iron needed, which is 64.4 g.
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
Formula for iron iii sulfide?
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
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 equation for iron reacting with sulfur?
iron + sulphur -> iron sulphide Fe + S -> FeS
In the reaction 2 Fe plus 3 S--- Fe2S3 how much iron is required to react with 48.0 g of sulfur?
To determine the amount of iron required, you first need to find the molar mass of sulfur (32.06 g/mol) and the molar mass of iron (55.85 g/mol). Then, use the stoichiometry of the reaction to calculate the amount of iron needed, which is 64.4 g.
What does Fe2S3 break down into?
Iron(III) sulfide (Fe2S3) breaks down into iron(III) oxide (Fe2O3) and sulfur dioxide (SO2).
How many milliliters of 0.200 M FeCl3 are needed to react with an excess of Na2S to produce 0.690 g of Fe2S3 if the percent yield for the reaction is 65.0 3 Na2S(aq) plus 2 FeCl3(aq) Fe2S3(s) plus?
To find the moles of Fe2S3 produced, convert 0.690 g to moles using the molar mass of Fe2S3. Then, use the stoichiometry of the reaction to determine the moles of FeCl3 required. Finally, use the molarity of FeCl3 to calculate the volume in milliliters needed, keeping in mind the percent yield.
What type of reaction is Fe2S3 equals 2Fe plus 3S?
decomposition
Metallic Iron was heated with solid sulfur to form a single solid sulphate what is the balanced chemical reaction?
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)
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.
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 formula for iron IIIsulfide?
Iron has a charge of +3 and Sulfur has a charge of -2, so iron III sulfide is: Fe2S3
What type of bond is Fe2S3?
Fe2S3 is an ionic bond. Iron (Fe) typically forms cations with a +2 charge, while sulfur (S) typically forms anions with a -2 charge. When these two elements combine to form Fe2S3, they do so through an ionic bond where Fe3+ ions are attracted to S2- ions.
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 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
Formula for iron iii sulfide?
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
