Omar Bennett
Ammonia, with the chemical formula NH3, is an inorganic alkaline gas with a distinct pungent smell. Its molar mass is 17.04 g/mol, which means that 17.04 grams constitute one gram-molecular weight of ammonia. This is calculated by adding the atomic weights of nitrogen and three hydrogen atoms.
| Characteristics | Values |
|---|---|
| Molecular weight | 17.04 u |
| Molar mass | 17.04 g/mol |
| Mass of one molecule | 2.82 x 10^-23 grams |
| Formula | NH3 |
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What You'll Learn
- Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol)
- Molecular weight is calculated by adding the atomic weights of all atoms in a molecule
- One atomic mass unit is one-twelfth of the mass of a carbon-12 atom
- The formula weight is the weight of all atoms in a formula
- The molecular formula for ammonia is NH3
Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol)
Molar mass is a fundamental concept in chemistry that relates to the mass of a substance. It is defined as the mass of one mole of a substance, expressed in grams per mole (g/mol). This definition establishes a critical link between the mass of a substance and the number of particles it contains.
To understand molar mass, it is essential to grasp the concept of a mole. A mole is a unit of measurement in chemistry that represents a specific quantity of a substance. Specifically, one mole of a substance contains a definite number of particles, known as Avogadro's number, which is approximately 6.022 x 10^23 particles per mole. This concept allows chemists to work with very large numbers of atoms and molecules typically found in everyday quantities of substances.
The significance of molar mass lies in its ability to bridge the microscopic world of atoms and molecules with the macroscopic world of grams and litres. By expressing the mass of a substance in grams per mole, chemists can perform stoichiometry calculations and predict how substances will react with each other in terms of mass and the number of moles. This is particularly useful when dealing with macroscopic or weighable quantities of a substance.
To calculate the molar mass of a substance, you need to consider its chemical formula and the atomic weights of its constituent atoms. For example, in the case of ammonia (NH3), you would sum the atomic weights of nitrogen (N) and hydrogen (H). Nitrogen has an atomic weight of 14.01 u, and hydrogen has an atomic weight of 1.01 u. Thus, the molar mass of ammonia is (14.01 u + 3(1.01 u)) = 17.04 u, which corresponds to 17.04 g/mol.
It is important to distinguish molar mass from molecular mass or molecular weight. While molar mass refers to the average molecular mass of all molecules in a sample, molecular mass represents the mass of one molecule of a specific isotopic composition. Additionally, molar mass is expressed in grams per mole (g/mol), while molecular mass is typically measured in unified atomic mass units (u) or daltons (Da).
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Molecular weight is calculated by adding the atomic weights of all atoms in a molecule
The molecular weight of a substance is calculated by adding up the atomic weights of all the atoms in a molecule of that substance. Each element on the periodic table has a unique atomic weight, which is the average mass of atoms of that element, accounting for the different isotopes and their respective abundances. These atomic weights are expressed in unified atomic mass units (u), where one atomic mass unit is defined as one-twelfth of the mass of a carbon-12 atom.
For example, let's consider the calculation of the molecular weight of water (H2O). Water has two hydrogen atoms and one oxygen atom. Hydrogen has an atomic weight of 1 u, and oxygen has an atomic weight of 16 u. Therefore, the molecular weight of water is 18 u (2 x 1 u + 1 x 16 u).
The molecular weight of ammonia (NH3) can be calculated in a similar way. Ammonia has one nitrogen atom and three hydrogen atoms. Nitrogen has an atomic weight of 14.01 u, and hydrogen has an atomic weight of 1.01 u. Therefore, the molecular weight of ammonia is 17.04 u (1 x 14.01 u + 3 x 1.01 u). This also corresponds to a molar mass of 17.04 g/mol.
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is numerically equivalent to the molecular weight but expressed in different units. Molar mass is useful because it relates the mass of a substance to the number of particles it contains, as per Avogadro's number.
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One atomic mass unit is one-twelfth of the mass of a carbon-12 atom
The molar mass of a substance is the mass of one mole of that substance, usually expressed in grams per mole (g/mol). It is numerically equivalent to the molecular weight but expressed in different units. Molar mass is calculated by summing the atomic weights of all atoms in a molecule. For example, the molecular weight of ammonia (NH3) is 17.04 u, which corresponds to a molar mass of 17.04 g/mol.
Atomic weights are expressed in unified atomic mass units (u), where one atomic mass unit (amu) is defined as one-twelfth of the mass of a carbon-12 atom. Carbon-12 was chosen as the standard because it is the most abundant isotope of carbon. It provides an average value that fits well with the rest of the elements. While the mass of a proton can be measured quite precisely, the mass of carbon-12 is slightly less than the weight of six protons and six neutrons. This is because the mass lost by the atom when its protons and neutrons come together to form a nucleus is equivalent to the binding energy of the nucleus.
The use of carbon-12 as the standard also takes into account the energetic nature of atomic reactions, where the energy involved becomes significant compared to the masses of the particles involved. In chemical reactions, the energy lost is about 1 in a million of the original mass, but in nuclear reactions, it can be as high as a few percent. The choice of carbon-12 as the standard was a good compromise for earlier definitions.
The molecular weight of a substance is calculated by summing the atomic weights of all atoms within a molecule. For example, the molecular weight of water (H2O) is the weight of two hydrogen atoms plus the weight of one oxygen atom, or approximately 18 u (2(1 u) + 16 u). This calculation is essential for accurate measurements in chemistry, such as determining the mass of a specific number of molecules.
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The formula weight is the weight of all atoms in a formula
The formula weight of a substance is the sum of the atomic weights of each atom in its chemical formula. It is expressed in units of atomic mass units (amu) or daltons (Da). For example, the formula weight of water (H2O) is calculated by adding the atomic weights of its constituent atoms: 2 x (1.0079 amu) + 1 x (15.994 amu) = 18.01528 amu.
Ammonia has the chemical formula NH3, meaning it contains one nitrogen atom and three hydrogen atoms. To calculate the formula weight of ammonia, we need to find the atomic weights of nitrogen and hydrogen. Nitrogen has an atomic weight of 14.01 u (unified atomic mass units), while hydrogen has an atomic weight of 1.01 u. Adding these weights together gives us the molecular weight of ammonia: 14.01 u + 3(1.01 u) = 17.04 u. This also corresponds to a molar mass of 17.04 g/mol, which is the mass of one mole of ammonia.
Molar mass is a crucial concept in chemistry, as it allows scientists to predict how substances will react with each other in terms of mass and the number of moles. It is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). Molar mass is particularly useful because it relates the mass of a substance to the number of particles it contains, as per Avogadro's number.
Formula weights are especially valuable in determining the relative weights of reagents and products in a chemical reaction. They are calculated using the chemical formula of the compound and the periodic table of elements. By adding up the atomic weights of all atoms in the formula, we can determine the formula weight or molecular weight of the substance. This calculation is essential for accurate measurements and understanding the properties of chemical compounds.
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The molecular formula for ammonia is NH3
Ammonia, with the molecular formula NH3, is an inorganic chemical compound of nitrogen and hydrogen. It is a stable binary hydride and the simplest pnictogen hydride. In its pure form, ammonia is a colourless gas with a pungent smell. It is biologically considered a common nitrogenous waste and is used as a precursor to fertilisers.
The molecular formula of a compound is a representation of the number and type of atoms that constitute the compound. In the case of ammonia, its molecular formula, NH3, indicates that each molecule of ammonia contains one nitrogen atom and three hydrogen atoms.
The molecular formula is also essential for calculating the molar mass and molecular weight of a compound. Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is numerically equivalent to the molecular weight but expressed in different units. To calculate the molar mass of ammonia, we need to determine the combined atomic weights of all the atoms in one molecule of ammonia.
Nitrogen has an atomic weight of approximately 14.01 u (unified atomic mass units), while hydrogen has an atomic weight of approximately 1.01 u. By adding the atomic weights of one nitrogen atom and three hydrogen atoms, we can calculate the molecular weight of ammonia:
Molecular Weight = 14.01 u + 3(1.01 u) = 17.04 u
Since 1 u is equal to 1 g/mol, we can convert the molecular weight of ammonia from unified atomic mass units to grams per mole:
Molecular Weight = 17.04 g/mol
This measure is crucial in chemistry for stoichiometry calculations, as it allows scientists to predict how substances will react with each other in terms of mass and number of moles. It helps reconcile the microscale world of atoms and molecules with the macroscale world of grams and litres.
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Frequently asked questions
The molecular weight of ammonia (NH3) is 17.04 u.
The gram-molecular weight of ammonia, also known as its molar mass, is 17.04 g/mol.
To calculate the gram-molecular weight of ammonia, you need to add up the atomic weights of all the atoms in its chemical formula. For ammonia (NH3), this means adding the atomic weight of nitrogen (14.01 u) and three times the atomic weight of hydrogen (1.01 u). This gives a total of 17.04 u, which is also the molecular weight. Since 1 u is equal to 1 g/mol, the gram-molecular weight of ammonia is 17.04 g/mol.
Molecular weight and gram-molecular weight are numerically equivalent but expressed in different units. Molecular weight is expressed in atomic mass units (u), while gram-molecular weight, also known as molar mass, is expressed in grams per mole (g/mol).
