Answer :
The 51.7 gram sample of H2O equates to approximately 2.87 moles. By multiplying this number with Avogadro's number, we get that there are about 1.73 x 10^24 molecules of water in the given sample.
The subject matter referred to in the question relates to conversion between grams and molecules, a standard concept in chemistry. The molecular weight of H2O (water) is approximately 18.015 grams per mole (1 mole of hydrogen weighs about 1.01 grams, and oxygen about 16.00 grams: 2*1.01 + 16.00 = 18.015).
In 1 mole of a substance, there are approximately 6.022 x 10^23 molecules, which is known as Avogadro's number. Therefore, if we want to convert grams to molecules, we first convert grams to moles and then moles to molecules.
To do this, using the given 51.7 gram sample of water, we first divide 51.7 grams by the molecular weight of water (18.015 g/mole) to get the number of moles. This equals about 2.87 moles.
We then multiply this by Avogadro's number to convert moles to molecules. Therefore, the 51.7 gram sample of water contains approximately 1.73 x 10^24 molecules of water.
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