How many molecules are in 2.6 grams of H2O?
There are 6.022 x 10^23 molecules in a mole. How many moles do you have of water in 2.6 g? 2.6/molar mass = moles.
(6.022×10^23)×(2.6)/18
Well, let's see how we can "hydrate" your question with a splash of laughter! In order to calculate the number of molecules in 2.6 grams of H2O, we need to apply some "molecular comedy."
First, we need to determine the molar mass of water (H2O). Hydrogen (H) has a molar mass of approximately 1 gram/mol, while oxygen (O) has a molar mass of approximately 16 grams/mol. Since there are two hydrogen atoms and one oxygen atom in water, the total molar mass of water is about 18 grams/mol.
Now, let's do some "molecular scaling"! If we have 2.6 grams of H2O and the molar mass is 18 grams/mol, we can set up a proportion:
2.6 g / 18 g/mol = x mol / 1
Solving this proportion, we find that there are approximately 0.144 moles of H2O present.
Finally, we need Avogadro's constant to convert moles to molecules. Avogadro's constant, approximately 6.022 x 10^23, tells us the number of items in one mole.
Multiplying the number of moles (0.144) by Avogadro's constant, we find that there are approximately 8.67 x 10^22 molecules of H2O in 2.6 grams.
So, to answer your question, there are approximately 8.67 x 10^22 molecules of H2O in 2.6 grams. That's a lot of molecules to "water around" with!
To determine the number of molecules in a given mass of a substance, you can use the concept of moles and Avogadro's number. The steps to calculate this are as follows:
1. Find the molar mass of water (H2O). The molar mass of hydrogen (H) is approximately 1 gram/mole, and the molar mass of oxygen (O) is approximately 16 grams/mole. Therefore, the molar mass of water (H2O) is 1 + 1 + 16 = 18 grams/mole.
2. Calculate the number of moles in the given mass of water using the formula:
Moles = Mass / Molar mass
Substituting the known values:
Moles = 2.6 grams / 18 grams/mole
Moles = 0.1444 moles
3. Apply Avogadro's number. Avogadro's number (NA) is approximately 6.022 x 10^23 molecules/mole. Therefore, to calculate the number of molecules, multiply the number of moles by Avogadro's number:
Number of molecules = Moles x Avogadro's number
Number of molecules = 0.1444 moles x 6.022 x 10^23 molecules/mole
Number of molecules ≈ 8.7 x 10^22 molecules
Therefore, there are approximately 8.7 x 10^22 molecules in 2.6 grams of H2O.
To determine the number of molecules in a given amount of a substance, we need to use the concept of moles. A mole is a unit used in chemistry to represent a specified number of particles, which is approximately 6.022 x 10^23 particles, called Avogadro's number.
To solve this problem, we need to follow these steps:
Step 1: Determine the molar mass of H2O.
The molar mass of a compound can be calculated by summing up the atomic masses of its constituent elements. For H2O, the atomic masses of hydrogen (H) and oxygen (O) are approximately 1 gram/mole and 16 grams/mole, respectively.
So, the molar mass of H2O = (2 x 1 g/mol for hydrogen) + (1 x 16 g/mol for oxygen) = 2 + 16 = 18 g/mol.
Step 2: Calculate the number of moles of H2O.
To find the number of moles, we divide the given mass of the compound by its molar mass.
moles = mass (in grams) / molar mass
moles = 2.6 g / 18 g/mol ≈ 0.144 moles (rounded to three decimal places).
Step 3: Calculate the number of molecules.
Now, we can determine the number of molecules by multiplying the number of moles by Avogadro's number.
number of molecules = moles x Avogadro's constant
number of molecules = 0.144 moles x (6.022 x 10^23 molecules/mol)
number of molecules ≈ 8.68 x 10^22 molecules.
So, there are approximately 8.68 x 10^22 molecules in 2.6 grams of H2O.