0
What else can I help you with?
Given the following equation 8 Fe plus FeS what mass of iron is needed to react with 16.0g of sulfur?
To determine the mass of iron needed to react with 16.0g of sulfur, first balance the chemical equation: 8 Fe + FeS2 -> 9 FeS. As each Fe reacts with 1/2 S, the molar ratio is 8:1/2. Calculate the molar mass of Fe and FeS to convert between moles and grams. Then use the molar ratio to find the mass of Fe needed: (16.0g S)*(8 mol Fe / 1 mol S) * (55.85 g Fe / 1 mol Fe) = 711.2 g Fe.
How many grams of iron could be recovered from 75.89 g FeO?
To calculate the amount of iron that can be recovered from FeO, we need to consider the molar ratio between Fe and FeO. FeO consists of 1 iron atom and 1 oxygen atom. The molar mass of Fe is 55.85 g/mol, and the molar mass of FeO is 71.85 g/mol. By dividing the molar mass of Fe by the molar mass of FeO and multiplying by the given mass of FeO, we can determine the amount of iron that can be recovered.
Steel wool placed in sulfuric acid equation?
The reaction between steel wool (Fe) and sulfuric acid (H2SO4) produces iron sulfate (FeSO4), hydrogen gas (H2), and water (H2O). The balanced chemical equation for this reaction is: Fe + H2SO4 -> FeSO4 + H2 + H2O
What is the molar mass of Fe NO3 2?
The molar mass of Fe(NO3)2 (iron(II) nitrate) is calculated by adding the atomic masses of all the atoms in the formula: Fe (iron) has a molar mass of approximately 55.85 g/mol, N (nitrogen) has a molar mass of approximately 14.01 g/mol, and O (oxygen) has a molar mass of approximately 16.00 g/mol. Therefore, the molar mass of Fe(NO3)2 is around 179.86 g/mol.
How many unpaired electrons are present in the Fe(ox)(H2O)2 complex?
The Fe(ox)(H2O)2 complex has four unpaired electrons.
Given the following equation 8 Fe plus FeS what mass of iron is needed to react with 16.0g of sulfur?
To determine the mass of iron needed to react with 16.0g of sulfur, first balance the chemical equation: 8 Fe + FeS2 -> 9 FeS. As each Fe reacts with 1/2 S, the molar ratio is 8:1/2. Calculate the molar mass of Fe and FeS to convert between moles and grams. Then use the molar ratio to find the mass of Fe needed: (16.0g S)*(8 mol Fe / 1 mol S) * (55.85 g Fe / 1 mol Fe) = 711.2 g Fe.
What is the molecular weight of nitroprusside?
The molar mass of Nitroprusside:Na2[Fe(CN)5NO] is 261.92 g/mol (anhydrous)Na2[Fe(CN)5NO].[H2O]2 is 297.95 g/mol (as dihydrate)
How many grams of aluminum would be required to produce 550 g of Fe?
To produce 550 g of Fe, you would need the same amount of Al based on the balanced chemical equation of the reaction between Al and Fe. The molar ratio between Al and Fe is 2:3. Therefore, you would need (2/3) * 550 g of Al, which is approximately 367 g.
What is the mass in grams in 1.00 molar mass FE?
What is the chemical 'FE'. Do you mean 'Fe'. If so to answer your question . The molar mass of iron (Fe) is 55.845
How many grams of iron could be recovered from 75.89 g FeO?
To calculate the amount of iron that can be recovered from FeO, we need to consider the molar ratio between Fe and FeO. FeO consists of 1 iron atom and 1 oxygen atom. The molar mass of Fe is 55.85 g/mol, and the molar mass of FeO is 71.85 g/mol. By dividing the molar mass of Fe by the molar mass of FeO and multiplying by the given mass of FeO, we can determine the amount of iron that can be recovered.
Steel wool placed in sulfuric acid equation?
The reaction between steel wool (Fe) and sulfuric acid (H2SO4) produces iron sulfate (FeSO4), hydrogen gas (H2), and water (H2O). The balanced chemical equation for this reaction is: Fe + H2SO4 -> FeSO4 + H2 + H2O
What is the molar mass of Fe NO3 2?
The molar mass of Fe(NO3)2 (iron(II) nitrate) is calculated by adding the atomic masses of all the atoms in the formula: Fe (iron) has a molar mass of approximately 55.85 g/mol, N (nitrogen) has a molar mass of approximately 14.01 g/mol, and O (oxygen) has a molar mass of approximately 16.00 g/mol. Therefore, the molar mass of Fe(NO3)2 is around 179.86 g/mol.
How many grams of Al are needed to completely react with 135 g Iron?
To calculate the mass of aluminum (Al) needed to completely react with 135 g of iron, you first need to determine the molar ratio between them from the balanced chemical equation. The balanced equation for the reaction between aluminum and iron is 2Al + 3Fe2O3 -> 3Fe + Al2O3. From this ratio, you can calculate that 2 moles of aluminum (Al) react with 3 moles of iron (Fe). Next, calculate the molar mass of aluminum (Al) and use it to convert the given mass of iron to moles. Finally, use the molar ratio to find the mass of aluminum needed.
What is one difference between water and iron?
Water (H2O) is a chemical compound and iron (Fe) is a chemical element.
How many unpaired electrons are present in the Fe(ox)(H2O)2 complex?
The Fe(ox)(H2O)2 complex has four unpaired electrons.
What is the empirical formula of an iron oxide that 65.0 percent fe and 35.0 percent O?
The empirical formula of the iron oxide compound is Fe₂O₃. This is determined by dividing the percentage of each element by its molar mass to find the ratio of atoms in the compound.
What mass of carbon monoxide is needed to produce 143.9g of iron according to Fe2O3 3CO --2 Fe 3CO2?
To find the mass of carbon monoxide needed, we need to use the stoichiometric ratio between iron and carbon monoxide. From the balanced equation, we can see that 3 moles of carbon monoxide produce 2 moles of iron. First, calculate the molar mass of iron (Fe), which is 55.85 g/mol. Next, use the molar ratio between iron and carbon monoxide (2:3) to find the moles of carbon monoxide required. Finally, convert the moles of carbon monoxide to grams using its molar mass (28.01 g/mol).
