Let's calculate the mass of [tex]\(10.0 \, \text{mol} \, \text{CH}_2\text{O}_2\)[/tex].
To find out the mass, we need to use the formula:
[tex]\[ \text{Mass} = \text{Moles} \times \text{Molar Mass} \][/tex]
Given:
- Moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex] = [tex]\( 10.0 \, \text{mol} \)[/tex]
- Molar mass of [tex]\( \text{CH}_2\text{O}_2 \)[/tex] = [tex]\( 46.03 \, \text{g/mol} \)[/tex]
Using these values, we substitute into the formula:
[tex]\[ \text{Mass} = 10.0 \, \text{mol} \times 46.03 \, \text{g/mol} \][/tex]
So, the mass of [tex]\( 10.0 \, \text{mol} \, \text{CH}_2\text{O}_2 \)[/tex] is:
[tex]\[ \text{Mass} = 460.3 \, \text{g} \][/tex]
Thus, the number that goes in the green box is:
[tex]\[
3. \, 46.03 \, \text{g} \, \text{CH}_2\text{O}_2
\][/tex]
