How many molecules are there in a 42.3 g sample of water

Explanation:

In order to figure out how many molecules of water are present in that  

48.90-g

sample, you first need to determine how many moles of water you have there.

As you know, a mole is simply a very large collection of molecules. In order to have one mole of something, you need to have exactly  

6.022

⋅

10

23

molecules of that something - this is known as Avogadro's number.

In order to get to moles, you must use water's molar mass. A substance's molar mass tells you the mass of one mole of molecules of said substance.

Water has a molar mass of  

18.015 g/mol

. This means that one mole of water molecules has a mass of  

18.015 g

.

So, to sum this up,  

6.022

⋅

10

23

molecules of water will amount to  

1 mole

of water, which in turn will have a mass of  

18.015 g

.

a pan containing water is placed in a positio n where it is exposed to a 10 mile per hour wind. the pan contains a uniform depth of 1.27 cm of water, is quite wide, and has a length of 2.44 m in the wind direction. the water in the pan is at a constant temperature of 15.5 °c.

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.