Answered

IDNLearn.com: Where curiosity meets clarity and questions find their answers. Our community is here to provide the comprehensive and accurate answers you need to make informed decisions.

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

Let's begin by setting up our expression. Which number choice goes in the green box?

1. [tex]1 \text{ mole } CH_2O_2[/tex]

2. [tex]6.02 \times 10^{23} \text{ molecules } CH_2O_2[/tex]

3. [tex]46.03 \text{ g } CH_2O_2[/tex]

Sagot :

GinnyAnsweridn
To find the mass of [tex]\( 10.0 \)[/tex] moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex], we need to know the molar mass of the compound. The molar mass is found by adding the atomic masses of all atoms in the molecule. The molar mass of [tex]\( \text{CH}_2\text{O}_2 \)[/tex] is [tex]\( 46.03 \, \text{g/mol} \)[/tex].

We can use the molar mass to convert moles into grams. The expression we use is:
[tex]\[ \text{mass} = \text{moles} \times \text{molar mass} \][/tex]

In this case, the molar mass of [tex]\( 1 \, \text{mol CH}_2\text{O}_2 \)[/tex] is [tex]\( 46.03 \, \text{g} \)[/tex].

So, [tex]\(\text{mass} = 10.0 \, \text{mol} \times 46.03 \, \text{g/mol} = 460.3 \, \text{g} \)[/tex].

The number that goes in the green box is:
[tex]\[ 3. \, 46.03 \, \text{g CH}_2\text{O}_2 \][/tex]

Thus, the mass of [tex]\( 10.0 \)[/tex] moles of [tex]\( \text{CH}_2\text{O}_2 \)[/tex] is [tex]\( 460.3 \, \text{g} \)[/tex].
We are delighted to have you as part of our community. Keep asking, answering, and sharing your insights. Together, we can create a valuable knowledge resource. IDNLearn.com is your go-to source for accurate answers. Thanks for stopping by, and come back for more helpful information.