Answer :
Sure! Let's find the molecular formula step by step.
1. Identify the empirical formula and the scale factor:
- Empirical formula: [tex]\( \text{CH}_2\text{O} \)[/tex]
- Scale factor: 5
2. Extract the subscript (number of atoms) for each element in the empirical formula:
- Carbon (C): 1
- Hydrogen (H): 2
- Oxygen (O): 1
3. Apply the scaling factor to each element:
- For Carbon (C): [tex]\( 1 \times 5 = 5 \)[/tex]
- For Hydrogen (H): [tex]\( 2 \times 5 = 10 \)[/tex]
- For Oxygen (O): [tex]\( 1 \times 5 = 5 \)[/tex]
4. Write the molecular formula with the new subscripts:
- Molecular formula: [tex]\( \text{C}_5\text{H}_{10}\text{O}_5 \)[/tex]
So, the molecular formula is [tex]\( \text{C}_5\text{H}_{10}\text{O}_5 \)[/tex].
1. Identify the empirical formula and the scale factor:
- Empirical formula: [tex]\( \text{CH}_2\text{O} \)[/tex]
- Scale factor: 5
2. Extract the subscript (number of atoms) for each element in the empirical formula:
- Carbon (C): 1
- Hydrogen (H): 2
- Oxygen (O): 1
3. Apply the scaling factor to each element:
- For Carbon (C): [tex]\( 1 \times 5 = 5 \)[/tex]
- For Hydrogen (H): [tex]\( 2 \times 5 = 10 \)[/tex]
- For Oxygen (O): [tex]\( 1 \times 5 = 5 \)[/tex]
4. Write the molecular formula with the new subscripts:
- Molecular formula: [tex]\( \text{C}_5\text{H}_{10}\text{O}_5 \)[/tex]
So, the molecular formula is [tex]\( \text{C}_5\text{H}_{10}\text{O}_5 \)[/tex].
