The Molar Mass Of Ammonia { \left( NH_3 \right)$}$ Is 17 G. What Is The Number Of Moles And Volume In { Dm^3$}$ At Standard Temperature And Pressure (s.t.p) Occupied By 1.7 G Of Ammonia Molecules?A. 0.01 Mol And [$2.24 ,
Introduction
In chemistry, understanding the properties of molecules is crucial for various applications, including chemical reactions, stoichiometry, and gas laws. One of the fundamental properties of a molecule is its molar mass, which is the mass of one mole of the substance. In this article, we will explore the molar mass of ammonia (NH3) and use it to calculate the number of moles and volume occupied by a given mass of ammonia molecules at standard temperature and pressure (s.t.p).
The Molar Mass of Ammonia
The molar mass of ammonia (NH3) is 17 g/mol. This value is obtained by summing the atomic masses of nitrogen (N) and hydrogen (H) atoms. The atomic mass of nitrogen is 14 g/mol, and the atomic mass of hydrogen is 1 g/mol. Since ammonia has one nitrogen atom and three hydrogen atoms, its molar mass is calculated as follows:
Molar mass of NH3 = (1 x 14 g/mol) + (3 x 1 g/mol) = 17 g/mol
Calculating the Number of Moles
To calculate the number of moles of ammonia, we can use the formula:
Number of moles = mass of substance / molar mass
In this case, we are given a mass of 1.7 g of ammonia. We can plug this value into the formula to calculate the number of moles:
Number of moles = 1.7 g / 17 g/mol = 0.1 mol
Calculating the Volume Occupied by Ammonia
At standard temperature and pressure (s.t.p), one mole of an ideal gas occupies a volume of 22.4 liters or 22.4 dm^3. We can use this value to calculate the volume occupied by 0.1 mol of ammonia:
Volume = number of moles x 22.4 dm^3/mol = 0.1 mol x 22.4 dm^3/mol = 2.24 dm^3
Conclusion
In conclusion, the molar mass of ammonia is 17 g/mol. By using this value, we can calculate the number of moles and volume occupied by a given mass of ammonia molecules at standard temperature and pressure (s.t.p). In this article, we calculated the number of moles and volume occupied by 1.7 g of ammonia and found that it is 0.1 mol and 2.24 dm^3, respectively.
Applications of Molar Mass in Chemistry
The molar mass of a substance is a fundamental property that has numerous applications in chemistry. Some of these applications include:
- Stoichiometry: The molar mass of a substance is used to calculate the amount of substance required for a chemical reaction.
- Gas Laws: The molar mass of a gas is used to calculate the volume occupied by a given mass of gas at standard temperature and pressure (s.t.p).
- Chemical Reactions: The molar mass of a substance is used to calculate the amount of substance produced or consumed in a chemical reaction.
Limitations of Molar Mass
While the molar mass of a substance is a fundamental property, it has some limitations. Some of these limitations include:
- Ideal Gas Assumption: The molar mass of a substance is calculated assuming that the gas behaves ideally. However, real gases do not behave ideally, and their molar mass may not accurately reflect their actual behavior.
- Temperature and Pressure: The molar mass of a substance is calculated at standard temperature and pressure (s.t.p). However, the actual temperature and pressure of a substance may be different, which can affect its molar mass.
Conclusion
Q&A: The Molar Mass of Ammonia
Q: What is the molar mass of ammonia (NH3)?
A: The molar mass of ammonia (NH3) is 17 g/mol.
Q: How is the molar mass of ammonia calculated?
A: The molar mass of ammonia is calculated by summing the atomic masses of nitrogen (N) and hydrogen (H) atoms. The atomic mass of nitrogen is 14 g/mol, and the atomic mass of hydrogen is 1 g/mol. Since ammonia has one nitrogen atom and three hydrogen atoms, its molar mass is calculated as follows:
Molar mass of NH3 = (1 x 14 g/mol) + (3 x 1 g/mol) = 17 g/mol
Q: What is the relationship between the molar mass of a substance and its volume at standard temperature and pressure (s.t.p)?
A: At standard temperature and pressure (s.t.p), one mole of an ideal gas occupies a volume of 22.4 liters or 22.4 dm^3. This means that the volume occupied by a substance is directly proportional to the number of moles of the substance.
Q: How can the number of moles of a substance be calculated?
A: The number of moles of a substance can be calculated using the formula:
Number of moles = mass of substance / molar mass
For example, if we have 1.7 g of ammonia, we can calculate the number of moles as follows:
Number of moles = 1.7 g / 17 g/mol = 0.1 mol
Q: What is the volume occupied by 0.1 mol of ammonia at standard temperature and pressure (s.t.p)?
A: At standard temperature and pressure (s.t.p), one mole of an ideal gas occupies a volume of 22.4 liters or 22.4 dm^3. Therefore, the volume occupied by 0.1 mol of ammonia is:
Volume = number of moles x 22.4 dm^3/mol = 0.1 mol x 22.4 dm^3/mol = 2.24 dm^3
Q: What are some of the applications of molar mass in chemistry?
A: The molar mass of a substance has numerous applications in chemistry, including:
- Stoichiometry: The molar mass of a substance is used to calculate the amount of substance required for a chemical reaction.
- Gas Laws: The molar mass of a gas is used to calculate the volume occupied by a given mass of gas at standard temperature and pressure (s.t.p).
- Chemical Reactions: The molar mass of a substance is used to calculate the amount of substance produced or consumed in a chemical reaction.
Q: What are some of the limitations of molar mass?
A: While the molar mass of a substance is a fundamental property, it has some limitations, including:
- Ideal Gas Assumption: The molar mass of a substance is calculated assuming that the gas behaves ideally. However, real gases do not behave ideally, and their molar mass may not accurately reflect their actual behavior.
- Temperature and Pressure: The molar mass of a substance is calculated at standard temperature and pressure (s.t.p). However, the actual temperature and pressure of a substance may be different, which can affect its molar mass.
Conclusion
In conclusion, the molar mass of ammonia is 17 g/mol. By using this value, we can calculate the number of moles and volume occupied by a given mass of ammonia molecules at standard temperature and pressure (s.t.p). The molar mass of a substance has numerous applications in chemistry, including stoichiometry, gas laws, and chemical reactions. However, it has some limitations, including the ideal gas assumption and temperature and pressure effects.