Hydrogen is generated by passing hot steam over iron, which oxidizes to form Fe3O4, in the following equation:
a. if 625 g of Fe3O4 is produced in the reaction, how many moles of hydrogen are produced at the same time?
b. how many moles of iron would be needed to generate 27 g of hydrogen?
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To answer these questions, we need to use the molar masses of the substances involved in the reaction and apply stoichiometry. Here's how we can solve each part:
a. To find the number of moles of hydrogen (H2) produced when 625 g of Fe3O4 is generated, we'll follow these steps:
Step 1: Determine the molar mass of Fe3O4 (iron (III) oxide).
Using the periodic table, we can find the atomic masses of iron (Fe) and oxygen (O):
- Atomic mass of Fe = 55.845 g/mol
- Atomic mass of O = 16.00 g/mol
The molar mass of Fe3O4 can be calculated as follows:
Molar mass of Fe3O4 = (3 * Molar mass of Fe) + (4 * Molar mass of O)
Molar mass of Fe3O4 = (3 * 55.845 g/mol) + (4 * 16.00 g/mol)
Molar mass of Fe3O4 = 231.69 g/mol
Step 2: Convert the mass of Fe3O4 to moles.
To convert grams to moles, we'll use the formula:
Moles = Mass (g) / Molar mass (g/mol)
Number of moles of Fe3O4 = 625 g / 231.69 g/mol
b. To find the number of moles of iron (Fe) required to generate 27 g of hydrogen (H2), we'll follow these steps:
Step 1: Determine the molar mass of hydrogen (H2).
Using the periodic table, we find the atomic mass of hydrogen to be 1.008 g/mol.
Step 2: Convert the mass of hydrogen to moles.
Number of moles of H2 = 27 g / 1.008 g/mol
Please note that the molar mass of hydrogen is based on diatomic hydrogen (H2) since hydrogen gas is formed.
By following these steps, you can calculate the number of moles of hydrogen produced in part (a) and the number of moles of iron required in part (b).