If you began with 36 grams of water how many hydrogen and oxygen can you produce in a decomposition reaction

To determine the number of hydrogen and oxygen atoms that can be produced in a decomposition reaction, we need to know the chemical equation for the reaction. However, if we assume the reaction occurs based on the decomposition of water (H2O), we can proceed.

The molar mass of water (H2O) is approximately 18 grams/mol. It consists of two hydrogen (H) atoms with a molar mass of approximately 1 gram/mol each and one oxygen (O) atom with a molar mass of approximately 16 grams/mol.

To calculate the number of moles in 36 grams of water, we divide the mass by the molar mass:
Number of moles = mass / molar mass
Number of moles of water = 36 g / 18 g/mol = 2 moles of water

Since there are two moles of water, we can assume that there are 2 moles of hydrogen atoms and 1 mole of oxygen atoms in the 36 grams of water.

To determine the number of atoms in one mole of a substance, we use Avogadro's number, which is approximately 6.022 x 10^23. Therefore, we can multiply the number of moles by Avogadro's number to calculate the number of atoms.
Number of atoms = number of moles x Avogadro's number

For hydrogen, the number of atoms will be:
Number of hydrogen atoms = 2 moles x 6.022 x 10^23 = 1.2044 x 10^24 hydrogen atoms

For oxygen, the number of atoms will be:
Number of oxygen atoms = 1 mole x 6.022 x 10^23 = 6.022 x 10^23 oxygen atoms

Therefore, starting with 36 grams of water in a decomposition reaction, you can produce approximately 1.2044 x 10^24 hydrogen atoms and 6.022 x 10^23 oxygen atoms.