What is the mass in #3.01 * 10^23# molecules of #F_2#?

Answer 1

The answer to this is #1.14 * 10^25 grams #

To convert mol #F_2# to grams #F_2#, you simply have to multiply the given number of mol to the molar mass of the compound.

In this instance:

#g F_2 = (3.01 * 10^(23) mol) * (37.996 g/[mol] )#

#g F_2 = 1.1436796 * 10^(23)#

Using correct number of significant figures, #g F_2 = 1.14 * 10^25 grams #

note: molar mass of #F_2# means you have to multiply Fluorine's molar mass by 2.

molar mass of #F_2 = 2 * ( 18.992 g/[mol]) = 37.996 g/[mol] #

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Answer 2

Serenity Allen

To calculate the mass of (3.01 \times 10^{23}) molecules of (F_2), we first find the molar mass of (F_2), which is (38.00 , \text{g/mol}). Then, we convert the number of molecules to moles using Avogadro's number ((6.022 \times 10^{23}) molecules/mol). Finally, we multiply the number of moles by the molar mass to find the mass.

[ \text{Mass} = \left(3.01 \times 10^{23} \text{ molecules}\right) \times \left(\frac{1 \text{ mole}}{6.022 \times 10^{23} \text{ molecules}}\right) \times (38.00 , \text{g/mol}) ]

[ \text{Mass} = 19.99 , \text{g} ]

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.