Determine the mass of a sample of water containing 3.55×1022 molecules of h2o .

The relationship between the number of particles and the number of mole of a substance is given by the equation #N = n L#; where #N# is the number of particles, #n# is the number of mole, and #L# is Avogadro's constant.

#n# is also defined using the equation #n = frac(m)(M)#; where #m# is the mass and #M# is the molar mass of the substance.

Let's substitute the definition of #n# into the first equation:

#Rightarrow N = n L#

#Rightarrow N = frac(m)(M) times L#

Then, let's substitute the value of #N# and #L# into the equation:

#9.25 times 10^(22) = frac(m)(M) times 6.02 times 10^(23)#

Now, let's evaluate the molar mass of water:

#Rightarrow M(H_(2)O) = 2 times 1.00 + 16.0#

#Rightarrow M(H_(2)O) = 2.00 + 16.00#

#Rightarrow M(H_(2)O) = 18.00#

Substituting into the equation:

#Rightarrow 9.25 times 10^(22) = frac(m)(18.00) times 6.02 times 10^(23)#

Dividing both sides of the equation by #6.02 times 10^(23)#:

#Rightarrow 1.54 = frac(m)(18.00)#

Multiplying both sides by #18.00#:

#Rightarrow 27.72 = m#

#therefore m = 27.72#

Therefore, the mass of #9.25 times 10^(22)# molecules of water is #27.72##"g"#.

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