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TotalтВ╣0
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Calculate the molecular mass of ammonia, NH3тАЛ, using the provided atomic masses (Atomic mass of N=14┬аu and H=1┬аu).
21 u
10 u
42 u
17 u
17 u
The molecular mass of a compound is calculated by summing the atomic masses of all the individual atoms present in one molecule of the substance. For ammonia (NH3тАЛ), the molecule contains one nitrogen atom and three hydrogen atoms.
The molecular mass of a compound is calculated by summing the atomic masses of all the individual atoms present in one molecule of the substance. For ammonia (NH3тАЛ), the molecule contains one nitrogen atom and three hydrogen atoms.
Think of it like calculating the total weight of a basket: you add the weight of the fruit inside (nitrogen) plus the weight of the individual apples (hydrogen) to get the total.
NтВГH (N=14, H=3*1=3, 14+3=17)
Molecular┬аmass=тИС(Number┬аof┬аatoms┬аof┬аelement├ЧAtomic┬аmass┬аof┬аelement)
The principle of conservation of mass states that the total mass of a molecule is the sum of its constituents. For NH3тАЛ, we use the given atomic masses: mass of Nitrogen (N) = 14u and mass of Hydrogen (H) = 1u. Therefore, the total molecular mass is calculated as 1├Ч(Atomic┬аmass┬аof┬аN)+3├Ч(Atomic┬аmass┬аof┬аH).
Atomic mass unit (u) is a standard unit used to express the mass of atoms and molecules.
The subscript in a chemical formula indicates the number of atoms of that element present in the molecule.
For ammonia (NH3тАЛ), there is 1 atom of N and 3 atoms of H.
Provides a simple method to quantify the mass of molecules.
Assumes perfect integer values for atomic masses which may vary slightly in practice due to isotopes.
Determining molar mass for stoichiometry in chemical reactions.
Calculating the number of moles in a given mass of a substance.
Ammonia is a colorless, pungent gas widely used in fertilizers and industrial processes.
Calculation: 1├Ч14+3├Ч1=14+3=17u.
Options 21 u, 10 u, and 42 u are incorrect arithmetic results.
D is correct тАФ The molecular mass of ammonia (NH3тАЛ) is calculated as 14+(3├Ч1)=17u.
Always verify the subscripts in a chemical formula before multiplying by the atomic masses; missing a coefficient is the most common error in these calculations.
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