Question #b64d1

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Question #b64d1

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Answer 1 · 2017-07-31T09:23:34

MW is 18 grams per mol (for water). In 27 grams of water there are $9.03 \times 10^{23}$ $9.03times10^23$ molecules of water.

Explanation:

Water has molecular weight of 18 grams per mol (remember that hydrogen atomic weight is 1 and oxygen atomic weight is 16 grams and water formula is $H_{2} O$ $H_2O$ ).

1 mole of water contains $6.02 \times 10^{23}$ $6.02times10^23$ molecules.

If you have 27 grams of water, it means you have $\frac{27}{18} = 1.5$ $27/18 = 1.5$ moles of water.

If you have 1.5 moles of water, it means $1.5 \times 6.02 \times 10^{23}$ $1.5times6.02times10^23$ water molecules are in it.

When you do the multiplication, you will get

1.5 moles of water contain $9.03 \times 10^{23}$ $9.03times10^23$ molecules of water.

Answer 2 · 2017-07-31T12:09:38

$9.03 \times 10^{23} Molecules$ $9.03 xx 10^23 "Molecules"$

Explanation:

Recall $\to no of moles = \frac{No of Entity}{Avogadro Constant}$ $-> "no of moles" = "No of Entity"/"Avogadro Constant"$

Also $\to no of moles = \frac{mass}{molar mass}$ $-> "no of moles" = "mass"/"molar mass"$

Water $\to H_{2} O$ $-> H_2O$

$Mass of x H_{2} O \to 27 g$ $"Mass of" color(white)(x) H_2O -> 27g$

$Molar mass of x H_{2} O \to (1 \times 2) + 16 = 2 + 16 = 18 g m o l^{- 1}$ $"Molar mass of" color(white)(x) H_2O -> (1 xx 2) + 16 = 2 + 16 = 18gmol^-1$

$:. "no of moles of" color(white)(x) H_2O = (27cancelg)/(18cancelgmol^-1)$

$"no of moles of" color(white)(x) H_2O = 1.5mols$

But $"No of Entity" = "no of moles" xx "Avogadro Constant"$

Hence $"No of Entity (Molecules)" = 1.5 xx 6.02 xx 10^23$

$"No of Entity (Molecules)" = 9.03 xx 10^23 "Molecules"$

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