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What is the mass of [tex]$10.0 \, \text{mol} \, CH_2O_2$[/tex]?

Given:
[tex]\[
\begin{tabular}{c|c}
$10.0 \, \text{mol} \, CH_2O_2$ & $46.03 \, \text{g} \, CH_2O_2$ \\
\hline
& $1 \, \text{mol} \, CH_2O_2$ \\
\end{tabular}
\][/tex]

Calculate the mass of [tex]CH_2O_2[/tex].

Sagot :

GinnyAnsweridn
To determine the mass of 10.0 moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex], we can use the molar mass of the compound. The molar mass is the mass of one mole of a substance, which is given in grams per mole (g/mol). According to the provided information:

- The molar mass of [tex]\( \text{CH}_2\text{O}_2 \)[/tex] is [tex]\( 46.03 \, \text{g/mol} \)[/tex].

We also know that we have [tex]\( 10.0 \)[/tex] moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex].

To find the total mass of [tex]\( 10.0 \)[/tex] moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex], we use the relationship:

[tex]\[ \text{Mass} = \text{Number of Moles} \times \text{Molar Mass} \][/tex]

Plugging in our values:

[tex]\[ \text{Mass} = 10.0 \, \text{moles} \times 46.03 \, \text{g/mol} \][/tex]

[tex]\[ \text{Mass} = 460.3 \, \text{g} \][/tex]

Therefore, the mass of [tex]\( 10.0 \)[/tex] moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex] is [tex]\( 460.3 \, \text{g} \)[/tex].
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