How many grams in 1.61 x 1023 molecules of water (H2O)
1 answer:
Taking into account the definition of Avogadro's number and molar mass, 4.806 grams of water are present in 1.61×10²³ molecules.
<h3>Definition of Avogadro's Number</h3>Avogadro's Number or Avogadro's Constant is called the number of particles that make up a substance (usually atoms or molecules) and that can be found in the amount of one mole of said substance. Its value is 6.023×10²³ particles per mole. Avogadro's number applies to any substance.
<h3>Definition of molar mass</h3>The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.
<h3>Mass of water</h3>Taking into account the definition of Avogadro's Number, you can apply the following rule of three: if 6.023×10²³ molecules are contained in 1 mole of water, then 1.61×10²³ molecules are contained in how many moles of water?
amount of moles of water= (1.61×10²³ molecules× 1 mole)÷ 6.023×10²³ molecules
<u><em>amount of moles of water= 0.267 moles</em></u>
Now, taking into account the definition of molar mass, and knowing that the molar mass of water is 18 g/mole, you can apply the following rule of three: If by definition of molar mass 1 mole of the compound contains 18 grams, 0.267 moles of the compound contains how much mass?
<u><em>mass= 4.806 grams</em></u>
Finally, 4.806 grams of water are present in 1.61×10²³ molecules.
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