Chem Question Decomposition of Water

Liters of Hydrogen gas and oxygen gas produced when 50g of water decomposed
molecular weight of water = 18.02
any gas occupies 22.4 L per mole
show work pls!! :)

Chemical Equation is: 2H2O ====> 2H2 + O2

1. Solve for moles of H2O from the mass provided:

moles of H2O = 50 g / 18.02 g/mol = 2.77 moles

2. Calculate for the moles of H2 gas produced. Based on the given balanced chemical equation, 2 moles of H2O will produced 2 moles of H2. (Ratio is 2 : 2)

moles of H2 produced = moles of H2O x Ratio
moles of H2 produced = 2.77 moles x (2 moles H2 / 2 moles H2O)
moles of H2 produced = 2.77 moles H2

2. Calculate for the moles of O2 gas produced. Based on the given balanced chemical equation, 2 moles of H2O will produced 1 mole of O2. ( Ratio is 1 : 2 )

moles of O2 produced = moles of H2O x Ratio
moles of O2 produced = 2.77 moles x (1 moles O2 / 2 moles H2O)
moles of O2 produced = 1.385 moles O2

3. Multiply moles of H2 and O2 in 22.4 L per mole to get L of O2 and H2 produced:

L of H2 = (22.4 L / mole) x 2.77 mole = 62.048 L =====> answer

L of O2 = (22.4 L / mole) x 1.385 mole = 31.024 L ====> answer

If 18 gm is decomposed, 2gm H2[1mole= 22.4 lit [at NTP] & 1/2 mole=22.4/2 O2 are obtained.
Now you can get the volumes from as many as you want , as you know every 18 gm contributes these !