How many molecules does water have

1 answer:

8 0

So, we calculate how many molecules there are in a drop of water, which we determined contains 0.002775 moles: molecules in a drop of water = (6.022 x 1023 molecules/mole) x 0.002275 moles. molecules in a drop of water = 1.67 x 1021 water molecules.

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You have prepared a saturated solution of x at 20∘c using 39.0 g of water. how much more solute can be dissolved if the temperat

AleksAgata [21]

for 39g water solute dissolved at 20C = solubility ( g/ 100 g H2O ) × mass of water = ( 11g / 100g H2O ) × 39g H2O = 4.29 g

amount of solute dissolved at 30 C =

= 23 / 100 * 39 = 8.97 g

Amount of extra solute dissolved = 8.97 - 4.29 = 4.7 g

3 0

3 years ago

There are two common oxides of copper; one is 80% copper and the other is 89% copper by weight. Calculate the formula and name e

irakobra [83]

80% copper (Cu)

Cu: 80 : 63.546 = 1.259

O: 20 : 16 = 1.25

Cu:O = 1 : 1

the formula: CuO

89% copper (Cu)

Cu: 89 : 63.546 = 1.4

O: 11 : 16 = 0.6875

Cu:O = 2:1

the formula: Cu₂O

8 0

2 years ago

In ionic compounds, ________ lose their valence electrons to form positively charged ________. nonmetals, anions metals, polyato

Keith_Richards [23]

Answer:
In ionic compounds, Metals lose their valence electrons to form positively charged Cations.

Explanation:
Metals have the ability to loose elctrons readily. For example metals of Group IA and Group IIA readily looses electrons in order to obtain Noble Gas Configuration. On the other hand Non-metals tends to gain electrons and acquire negative charge. While Ions are made when an an element gain or loose electrons. After loosing electrons element get positive charge which is called as Cation while on gaining electron it gets negative charge called as Anion.

6 0

3 years ago

Read 2 more answers

A tetraphenyl phosphonium chloride (TPPCl) powder (FW=342.39) is 94.0 percent pure. How many grams are needed to prepare 0.45 L

slega [8]

Answer:

5.41 g

Explanation:

Considering:

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$