The following reaction represents the decomposition of hydrogen peroxide:

Balanced equation: 2H2O2 -> O2 + 2H2O

How many moles of oxygen are produced from the decomposition of 3.4g of hydrogen peroxide?

How many molecules of O2 are produced?

For the second question, is the answer 1 molecule?

2H2O2 ==> 2H2O + O2

3.4g is how many moles of H2O2? That is moles = grams/molar mass.
The equation tells you that 1 mole O2 is produced by 2 moles H2O2.

For the last part, no, 1 is not the answer. Remember there are 6.022E23 molecules in 1 mole.

Thank you!

For the second question could you tell me how to find the answer?

# molecules = mols O2 x 6.022E23 = ?

To determine how many moles of oxygen (O2) are produced from the decomposition of 3.4g of hydrogen peroxide (H2O2), we need to use the balanced equation and molar masses.

1. Calculate the molar mass of hydrogen peroxide (H2O2):
- Hydrogen (H) has a molar mass of approximately 1 gram/mole
- Oxygen (O) has a molar mass of approximately 16 grams/mole
- Multiply the molar mass of hydrogen by 2 and add it to the molar mass of oxygen: (2 * 1 g/mol) + (2 * 16 g/mol) = 2 g/mol + 32 g/mol = 34 g/mol

2. Convert the given mass of hydrogen peroxide (3.4g) to moles:
- Divide the mass of hydrogen peroxide by its molar mass: 3.4 g / 34 g/mol = 0.1 moles

3. Apply the stoichiometric ratio from the balanced equation to determine the number of moles of oxygen:
- According to the balanced equation, 2 moles of hydrogen peroxide produce 1 mole of oxygen: 2H2O2 -> O2 + 2H2O
- Multiply the number of moles of hydrogen peroxide (0.1 moles) by the stoichiometric ratio: 0.1 moles * (1 mole O2 / 2 moles H2O2) = 0.05 moles O2

Therefore, the decomposition of 3.4g of hydrogen peroxide produces 0.05 moles of oxygen.

As for the second question, we can calculate the number of molecules of oxygen produced from the number of moles obtained earlier.

4. Utilize Avogadro's number:
- Avogadro's number states that 1 mole of any substance contains 6.022 x 10^23 molecules.
- Multiply the number of moles of oxygen (0.05 moles from step 3) by Avogadro's number: 0.05 moles * 6.022 x 10^23 molecules/mole = 3.011 x 10^22 molecules

Therefore, the decomposition of 3.4g of hydrogen peroxide produces approximately 3.011 x 10^22 molecules of oxygen (O2).

Hence, the answer to the second question is not 1 molecule but rather approximately 3.011 x 10^22 molecules of O2.