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Calculate The Molecular Mass Of HNO3

Molecular Mass Calculation:

\[ \text{Molecular Mass} = (1.008 \times 1) + (14.01 \times 1) + (16.00 \times 3) = 63.018 \text{ g/mol} \]

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1. What is Molecular Mass?

Molecular mass (molecular weight) is the sum of the atomic masses of all the atoms in a molecule. It's typically expressed in atomic mass units (u) or grams per mole (g/mol).

2. How is Molecular Mass Calculated?

The molecular mass is calculated by summing the atomic masses of each element multiplied by the number of atoms of that element in the molecule:

\[ \text{Molecular Mass} = \sum (\text{Atomic Mass} \times \text{Number of Atoms}) \]

For HNO3 (Nitric Acid):

Calculation: (1.008 × 1) + (14.01 × 1) + (16.00 × 3) = 63.018 g/mol

3. Importance of Molecular Mass

Details: Molecular mass is crucial for stoichiometric calculations, preparing molar solutions, determining empirical formulas, and understanding reaction yields in chemistry.

4. Using the Calculator

Tips: Enter the number of atoms for each element in the molecule. The calculator will sum the atomic masses. Default values show the calculation for HNO3.

5. Frequently Asked Questions (FAQ)

Q1: What's the difference between molecular mass and molar mass?
A: They are numerically identical but molar mass refers to one mole of substance (g/mol) while molecular mass is the mass of one molecule (u).

Q2: How accurate are these atomic masses?
A: These are average atomic masses accounting for natural isotope abundance. For precise work, use exact isotopic masses.

Q3: Can I calculate formula mass for ionic compounds?
A: Yes, the same principle applies to ionic compounds (called formula mass rather than molecular mass).

Q4: Why is molecular mass important in solutions?
A: It's used to prepare molar solutions where 1 mole = molecular mass in grams dissolved in 1 liter of solution.

Q5: How does this relate to the ideal gas law?
A: Molecular mass is used to convert between mass and moles in gas law calculations (PV = nRT).

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