The following reaction represents the decomposition of hydrogen peroxide:
2H2O2 -> O2 (g) + 2H2O (l)
How many molecules of water are produced from the decomposition of 3.4g of hydrogen peroxide, H2O2?
Please help, I got 0.02 molecules of water but need to verify my answer (not sure I did this right).
I'm not understanding. what do you mean figure the moles of H2O2 in 3.4 g of water? You get the same number of moles of water? I calculated:
nH2O2 = 3.4g/34.02g/mol= 0.0999412 mol
Water on the other hand has 18.02 mol
sorry but I'm not understanding. I think for this particular answer I need help from the beginning because I can't wrap my head around what I'm doing.
To determine the number of water molecules produced from the decomposition of 3.4g of hydrogen peroxide, we need to use the molar masses and stoichiometry of the reaction.
1. Start by calculating the molar mass of hydrogen peroxide (H2O2).
The molar mass of hydrogen (H) is 1.008 g/mol, and the molar mass of oxygen (O) is 16.00 g/mol.
H2O2 consists of 2 hydrogen atoms and 2 oxygen atoms, so the molar mass is:
(2 * 1.008 g/mol) + (2 * 16.00 g/mol) = 34.016 g/mol.
2. Convert the given mass of hydrogen peroxide (3.4g) to moles.
Moles = Mass / Molar mass
Moles = 3.4g / 34.016 g/mol = 0.1 mol (rounded to one decimal place).
3. Use the stoichiometric coefficients from the balanced equation to determine the moles of water produced.
The balanced equation tells us that 2 moles of hydrogen peroxide produce 2 moles of water.
So, the 0.1 mol of hydrogen peroxide will produce 0.1 mol of water.
4. Convert the moles of water to molecules.
To convert from moles to molecules, we use Avogadro's number, which is 6.022 x 10^23 molecules/mol.
Molecules = Moles * Avogadro's number
Molecules = 0.1 mol * 6.022 x 10^23 molecules/mol = 6.022 x 10^22 molecules.
Therefore, the correct answer is that 6.022 x 10^22 molecules of water are produced from the decomposition of 3.4g of hydrogen peroxide. Your initial answer of 0.02 molecules is incorrect.
To determine the number of molecules of water produced from the decomposition of 3.4g of hydrogen peroxide, you would need to follow a step-by-step process.
Step 1: Find the molar mass of hydrogen peroxide (H2O2)
The molar mass of hydrogen peroxide (H2O2) can be calculated by adding up the atomic masses of its constituent atoms. Hydrogen has a molar mass of around 1g/mol, and oxygen has a molar mass of around 16g/mol. Since there are two hydrogen atoms and two oxygen atoms in hydrogen peroxide, the molar mass of H2O2 is:
(2 x 1g/mol) + (2 x 16g/mol) = 34g/mol
Step 2: Calculate the number of moles of hydrogen peroxide
To determine the number of moles of hydrogen peroxide, divide the given mass (3.4g) by the molar mass of H2O2:
Number of moles = Given mass / Molar mass
Number of moles = 3.4g / 34g/mol
Number of moles = 0.1 mol
Step 3: Use the balanced equation to determine the stoichiometry
According to the balanced equation:
2H2O2 -> O2 (g) + 2H2O (l)
we can see that for every 2 moles of hydrogen peroxide that decomposes, 2 moles of water are produced.
Step 4: Calculate the number of moles of water produced
Since the stoichiometry states that for every 2 moles of hydrogen peroxide, 2 moles of water are produced, and we have 0.1 mole of hydrogen peroxide, we can conclude that 0.1 mole of water is produced.
Step 5: Convert moles of water to molecules of water
To convert moles to molecules, we use Avogadro's number, which is approximately 6.022 x 10^23 molecules/mol.
Number of molecules = Number of moles x Avogadro's number
Number of molecules = 0.1 mol x 6.022 x 10^23 molecules/mol
Number of molecules = 6.022 x 10^22 molecules
So the correct answer is 6.022 x 10^22 molecules of water produced from the decomposition of 3.4g of hydrogen peroxide (H2O2).
Therefore, your answer of 0.02 molecules of water is incorrect.
figure the moles of H2O2 in 3.4g
You get the same number of moles of water.
molecules= moleswater*avagradros number
No, the number of molecules is a very large number. You need to think on this. How can the answer be less than one molecule (as in .02 molecules)>