3fe+H2O----Fe3O+4H2
how many grams of steam and iron mist reat to produce 375g of magnetic iron oxide
Here is a solved example of a stochiomtry problem. Just follow the steps to solve this one.
http://www.jiskha.com/science/chemistry/stoichiometry.html
...and note that you need to balance the starting equation, i.e. it is not balanced as written above.
i think that it is 3 grams of Googaw reat
To determine how many grams of steam and iron mist are required to produce 375g of magnetic iron oxide (Fe3O4), we can use the balanced chemical equation you provided.
The equation is:
3Fe + H2O → Fe3O4 + 4H2
To solve the problem, we need to follow these steps:
Step 1: Determine the molar masses of water (H2O) and magnetic iron oxide (Fe3O4).
- The molar mass of H2O is calculated by adding the atomic masses of hydrogen (H) and oxygen (O), which are approximately 1g/mol and 16g/mol, respectively. Therefore, the molar mass of H2O is 18g/mol.
- The molar mass of Fe3O4 is calculated by adding the atomic masses of iron (Fe) and oxygen (O). The atomic mass of iron is approximately 56g/mol, and there are 4 oxygen atoms in Fe3O4 with a total atomic mass of approximately 64g/mol. Therefore, the molar mass of Fe3O4 is 160g/mol.
Step 2: Convert the given mass of magnetic iron oxide (Fe3O4) to moles.
- Divide the given mass (375g) by the molar mass of Fe3O4 (160g/mol):
375g / 160g/mol = 2.34 mol
Step 3: Use the stoichiometric ratio from the balanced equation to find the number of moles of H2O required.
- From the balanced equation, the stoichiometric ratio between Fe3O4 and H2O is 1:1. This means that for every 1 mole of Fe3O4, we need 1 mole of H2O.
- Therefore, the number of moles of H2O required is also 2.34 mol.
Step 4: Convert the number of moles of H2O to grams.
- Multiply the number of moles of H2O (2.34 mol) by the molar mass of H2O (18g/mol):
2.34 mol × 18g/mol = 42.12g
So, 42.12 grams of steam (H2O) and 42.12 grams of iron mist will react to produce 375 grams of magnetic iron oxide (Fe3O4).