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The page you've shared explains how to calculate the molecular formula of a compound from its molar mass using the empirical formula. Here's a breakdown of what's happening:

### **General Process**:
1. **Step 1: Calculate the Empirical Formula Mass**  
   - The empirical formula gives the simplest whole-number ratio of atoms in a compound. In this example, the empirical formula is \( \text{CH}_2\text{O} \).
   - The empirical formula mass is calculated by adding the atomic masses of the atoms in the empirical formula:  
     \( 12 \, \text{g/mol} \) for C, \( 2 \, \times \, 1 \, \text{g/mol} \) for H, and \( 16 \, \text{g/mol} \) for O.  
     Total = \( 30 \, \text{g/mol} \).

2. **Step 2: Calculate the Ratio**  
   - The molar mass (given as \( 180 \, \text{g/mol} \)) is divided by the empirical formula mass to find a ratio:  
     \( \frac{180}{30} = 6 \).
   - This ratio tells you how many times the empirical formula must be multiplied to get the molecular formula.

3. **Step 3: Find the Molecular Formula**  
   - Multiply each subscript in the empirical formula by the ratio found in Step 2.  
     In this case, the empirical formula \( \text{CH}_2\text{O} \) becomes \( \text{C}_6\text{H}_{12}\text{O}_6 \) because each subscript is multiplied by 6 (C: 1 × 6 = 6, H: 2 × 6 = 12, O: 1 × 6 = 6).

### **Final Molecular Formula**:  
The molecular formula is \( \text{C}_6\text{H}_{12}\text{O}_6 \), which is the formula for glucose.

Would you like any further details or have specific questions?

### 5 Related Questions:
1. What is the difference between empirical and molecular formulas?
2. How is the empirical formula determined if only percentages of elements are given?
3. Can a compound’s empirical formula and molecular formula ever be the same?
4. What role does molar mass play in determining the molecular formula?
5. How would you determine the molecular formula if given a different molar mass?

### Tip:
Always check that the ratio between molar mass and empirical formula mass is a whole number; if not, check your calculations or consider rounding.

This detailed guide walks you through calculating the molecular formula from a given empirical formula and molar mass. It includes step-by-step instructions on calculating the empirical formula mass, finding the ratio, and determining the molecular formula. Example: From CH2O to C6H12O6.

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