Answer :
To calculate the volume of 10.0 grams of gaseous ammonia (NH₃) at STP (Standard Temperature and Pressure), we can follow these steps:
1. Understand STP Conditions: At STP, one mole of any ideal gas occupies 22.4 liters.
2. Calculate the Molar Mass of Ammonia (NH₃):
- Nitrogen (N) has an atomic mass of about 14.01 g/mol.
- Hydrogen (H) has an atomic mass of about 1.01 g/mol, and there are three hydrogen atoms in NH₃.
- Therefore, the molar mass of NH₃ = 14.01 + (3 × 1.01) = 17.03 g/mol.
3. Determine the Number of Moles:
- We have 10.0 grams of NH₃.
- The number of moles = mass / molar mass = 10.0 grams / 17.03 g/mol ≈ 0.587 moles.
4. Calculate the Volume at STP:
- Since at STP, one mole of gas occupies 22.4 liters, the volume occupied by the moles of NH₃ we have is:
- Volume = number of moles × volume of one mole at STP
- Volume = 0.587 moles × 22.4 L/mol ≈ 13.2 L.
Therefore, the volume of 10.0 grams of gaseous ammonia at STP is approximately 13.2 liters. The correct answer is option (a).
1. Understand STP Conditions: At STP, one mole of any ideal gas occupies 22.4 liters.
2. Calculate the Molar Mass of Ammonia (NH₃):
- Nitrogen (N) has an atomic mass of about 14.01 g/mol.
- Hydrogen (H) has an atomic mass of about 1.01 g/mol, and there are three hydrogen atoms in NH₃.
- Therefore, the molar mass of NH₃ = 14.01 + (3 × 1.01) = 17.03 g/mol.
3. Determine the Number of Moles:
- We have 10.0 grams of NH₃.
- The number of moles = mass / molar mass = 10.0 grams / 17.03 g/mol ≈ 0.587 moles.
4. Calculate the Volume at STP:
- Since at STP, one mole of gas occupies 22.4 liters, the volume occupied by the moles of NH₃ we have is:
- Volume = number of moles × volume of one mole at STP
- Volume = 0.587 moles × 22.4 L/mol ≈ 13.2 L.
Therefore, the volume of 10.0 grams of gaseous ammonia at STP is approximately 13.2 liters. The correct answer is option (a).
