what mass of hydrogen was in an unknown compound containing only c, h, and o if 2.65kg H2O was produced by combustion analysis
2650g H2O x (2 molar mass H2/molar mass H2O) = ?
I need help
To determine the mass of hydrogen in the unknown compound, we can use the information provided about the mass of water produced during combustion analysis.
1. Start by noting that water (H2O) is made up of 2 hydrogen atoms and 1 oxygen atom.
2. Determine the molar mass of water:
- The molar mass of hydrogen (H) is approximately 1 g/mol.
- The molar mass of oxygen (O) is approximately 16 g/mol.
- Therefore, the molar mass of water (H2O) is approximately (2 * 1 g/mol) + (1 * 16 g/mol) = 18 g/mol.
3. Convert the mass of water produced (2.65 kg) to grams:
- 1 kg = 1000 g, so 2.65 kg is equal to 2.65 * 1000 g = 2650 g.
4. Calculate the number of moles of water produced:
- Divide the mass of water (2650 g) by the molar mass of water (18 g/mol):
2650 g / 18 g/mol ≈ 147.22 mol.
5. Since there are 2 moles of hydrogen in 1 mole of water, multiply the number of moles of water by 2 to find the moles of hydrogen:
- 147.22 mol * 2 = 294.44 mol.
6. Finally, calculate the mass of hydrogen:
- Multiply the moles of hydrogen (294.44 mol) by the molar mass of hydrogen (1 g/mol):
294.44 mol * 1 g/mol = 294.44 g.
Therefore, the mass of hydrogen in the unknown compound is approximately 294.44 grams.