How many atoms of hydrogen are contained in 1 mole of methane (CH4)?
Is it 3.01 x 10 to the 24th
How many water molecules are in a 0.649 g sample?
Answer in units of molecules.
1 mole of CH4 contains 6.02E23 molecules.
Each mols of CH4 has 4 mols H atoms.
What is 6.02E23 x 4 = ?
Then how many mols H2O are in 0.649 g? H2O. That's 0.649/18 = approx 0.04
Then approx 0.04 x 6.02E23 = H2O molecules in 0.649 g H2O. You should recalculate since my numbers are estimates
By the way how did you come by your answer for the first part?
To determine the number of atoms of hydrogen in 1 mole of methane (CH4), we need to understand the chemical formula for methane. The formula tells us that each methane molecule contains 1 carbon atom (C) and 4 hydrogen atoms (H).
To calculate the number of atoms in a mole of a substance, we use Avogadro's constant, which is approximately 6.022 x 10^23 atoms/mole.
So, in 1 mole of methane (CH4), we have 4 moles of hydrogen (H). Therefore, the number of atoms of hydrogen in 1 mole of methane is 4 multiplied by Avogadro's constant:
4 moles H x 6.022 x 10^23 atoms/mole = 2.4088 x 10^24 atoms of hydrogen
Therefore, the correct answer is 2.4088 x 10^24 atoms of hydrogen.
Moving on to the second question, to determine the number of water molecules in a 0.649 g sample, we need to use the molar mass of water and Avogadro's constant.
The molar mass of water (H2O) is approximately 18.015 g/mol.
First, we need to calculate the number of moles of water in the sample:
moles of water = mass of sample / molar mass of water
= 0.649 g / 18.015 g/mol
= 0.03599 mol (rounded to five decimal places)
Next, we can calculate the number of water molecules using Avogadro's constant:
number of water molecules = moles of water x Avogadro's constant
= 0.03599 mol x 6.022 x 10^23 molecules/mol
Therefore, the answer in units of molecules is approximately 2.170 x 10^22 water molecules.