A compound whose empirical formula is NO2 could have a molecular mass of what?
a) 23 b)39 c)92 d)120
0
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To determine the molecular mass of a compound with an empirical formula of NO2, we need to consider the atomic masses of nitrogen (N) and oxygen (O).
The atomic mass of nitrogen (N) is approximately 14.01 g/mol, and the atomic mass of oxygen (O) is approximately 16.00 g/mol.
The empirical formula NO2 tells us that there is one nitrogen atom and two oxygen atoms in each molecule of the compound. Thus, we can calculate the molecular mass by adding the atomic masses of the atoms in the formula:
(1 x Atomic mass of N) + (2 x Atomic mass of O)
= (1 x 14.01 g/mol) + (2 x 16.00 g/mol)
= 14.01 g/mol + 32.00 g/mol
= 46.01 g/mol
Therefore, the molecular mass of a compound with an empirical formula of NO2 is approximately 46.01 g/mol.
Based on the provided answer choices, none of the options match the calculated molecular mass of 46.01 g/mol. Therefore, none of the given options (a) 23, b) 39, c) 92, d) 120) are correct.
To determine the molecular mass of a compound with an empirical formula, we need to consider the atomic masses of the elements present in the compound.
The empirical formula NO2 indicates that there is one nitrogen atom (N) and two oxygen atoms (O) in the compound.
The atomic mass of nitrogen (N) is approximately 14 atomic mass units (amu) and the atomic mass of oxygen (O) is approximately 16 amu.
To calculate the molecular mass, we add together the atomic masses of the atoms present in the empirical formula.
Therefore, the molecular mass of the compound NO2 can be calculated as follows:
Molecular mass = (Atomic mass of N) + 2 × (Atomic mass of O)
= 14 + 2 × 16
= 14 + 32
= 46 amu
From the options given, the closest molecular mass to 46 amu is 39 amu. Therefore, the compound whose empirical formula is NO2 could have a molecular mass of 39 amu.
Thus, the correct answer is (b) 39.