Respuesta :
To determine the mass of each compound, we need to convert them into units of moles first. We use avogadros number to do this and use the molar mass of the compounds to convert to mass.
3.01 × 1023 molecules H2O ( 1 mole / 6.022x10^23 kg) (18.02 g / 1 mole) = 9.01 g
8.32 × 1020 formula units CaBr2 ( 1 mole / 6.022x10^23 kg) (199.89 g / 1 mole) = 0.28 g
1.93 × 1026 molecules XeF6 ( 1 mole / 6.022x10^23 kg) (245.28 g / 1 mole) = 78610.16 g
3.01 × 1023 molecules H2O ( 1 mole / 6.022x10^23 kg) (18.02 g / 1 mole) = 9.01 g
8.32 × 1020 formula units CaBr2 ( 1 mole / 6.022x10^23 kg) (199.89 g / 1 mole) = 0.28 g
1.93 × 1026 molecules XeF6 ( 1 mole / 6.022x10^23 kg) (245.28 g / 1 mole) = 78610.16 g
The molar mass of the substance is proportionate to the mass of the substance in grams to the moles of the substance.
9.01 g, 0.28 g and 78610.16 g is the mass for each of the sample.
How to calculate the mass?
Given,
- Molecules of [tex]\rm H_{2}O[/tex] = [tex]3.01 \times 10 ^{23}[/tex]
- Molecules of [tex]\rm CaBr_{2}[/tex] = [tex]8.32 \times 10^{20}[/tex]
- Molecules of [tex]\rm XeF_{6}[/tex] = [tex]1.93 \times 10^{26}[/tex]
Molar mass can be given by the formula,
[tex]\rm Molar \;mass = \dfrac{Mass}{Moles}[/tex]
For [tex]\rm H_{2}O[/tex]:
[tex]\begin{aligned}\rm Mass &= (\dfrac{3.01 \times 10^{23} \;\rm molecules}{6.022 \times 10^{23}})\times ({18.02\;\rm g})\\\\&=9.01 \;\rm g\end{aligned}[/tex]
For [tex]\rm CaBr_{2}[/tex]:
[tex]\begin{aligned}\rm Mass &= (\dfrac{8.32 \times 10^{20} \;\rm molecules}{6.022 \times 10^{23}})\times ({199.89\;\rm g})\\\\&=0.28 \;\rm g\end{aligned}[/tex]
For [tex]\rm XeF_{6}[/tex]:
[tex]\begin{aligned}\rm Mass &= (\dfrac{1.93 \times 10^{26} \;\rm molecules}{6.022 \times 10^{23}})\times ({245.28\;\rm g})\\\\&=78610.16 \;\rm g\end{aligned}[/tex]
Therefore, 9.01 g, 0.28 g and 78610.16 g is the mass for each of the sample.
Learn more about mass and molar mass here:
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