How To Calculate Molar Mass Of Glucose

Glucose Formula: C₆H₁₂O₆

\[ \text{Molar Mass} = 6 \times 12.01 + 12 \times 1.008 + 6 \times 15.999 = 180.156 \text{ g/mol} \]

Molar Mass:

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1. What Is Molar Mass?

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). For chemical compounds, it's calculated by summing the atomic masses of all atoms in the molecule.

2. How To Calculate Molar Mass

The molar mass calculation formula:

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

For glucose (C₆H₁₂O₆):

Carbon (C): 6 atoms × 12.01 g/mol = 72.06 g/mol
Hydrogen (H): 12 atoms × 1.008 g/mol = 12.096 g/mol
Oxygen (O): 6 atoms × 15.999 g/mol = 95.994 g/mol
Total: 72.06 + 12.096 + 95.994 = 180.156 g/mol

Explanation: Each element contributes to the total mass based on its atomic mass and the number of atoms present in the molecule.

3. Glucose Molecular Structure

Details: Glucose (C₆H₁₂O₆) is a simple sugar and important carbohydrate in biology. Its molecular formula shows it contains 6 carbon atoms, 12 hydrogen atoms, and 6 oxygen atoms.

4. Step-by-Step Calculation

Steps:

Identify the chemical formula (C₆H₁₂O₆)
List all elements and their counts
Multiply each element count by its atomic mass
Sum all the products to get total molar mass
Express result in g/mol with appropriate precision

5. Frequently Asked Questions (FAQ)

Q1: Why is molar mass important in chemistry?
A: Molar mass is essential for stoichiometric calculations, preparing solutions, determining molecular formulas, and understanding chemical reactions.

Q2: What are the standard atomic masses used?
A: Standard atomic masses are based on the IUPAC values: C=12.01, H=1.008, O=15.999 g/mol, which account for natural isotope abundances.

Q3: How does glucose molar mass compare to other sugars?
A: Glucose and fructose both have molar mass 180.16 g/mol, while sucrose (table sugar) has 342.30 g/mol (C₁₂H₂₂O₁₁).

Q4: Can I calculate molar mass for any compound?
A: Yes, this method works for any chemical compound as long as you know the molecular formula and standard atomic masses.

Q5: Why do we use average atomic masses?
A: Most elements exist as mixtures of isotopes, so we use weighted averages that reflect natural abundance for accurate calculations.