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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.
When was Break Down Barriers created?
Break Down Barriers was created in 1983.
Why can't lipase break down starch?
Lipase can't break down maltose because it is meant to break down lipids. Maltose is a form of a carboydrate, which is broken down by maltase.
Does amylase break down tissue meat?
No, you need protease to break down meat.
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 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
Formula for ironIIIsulfide?
Formula: Fe2S3
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.
2 Fe + 3 S -> Fe2S3?
Fesub2 S
What is the correct name for the compound Fe2S3?
Ferrous Sulfide = Iron (III) Sulfide Both -> 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.
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 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 soluble?
Iron (III) sulfide is not soluble in water.
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.
