Gaseous hydrogen and oxygen can be prepared in the laboratory from the decomposition of gaseous water. the equation for the reaction is2h2o(g) --> 2h2(g)+o2(g)calculate how many grams of o2(g) can be produced from 42.6 grams of h2o(g).

75.5 g O₂ (g) can be produced from 42.6 g of H₂O (g)

Explanation:

1) Balanced chemical equation (given):

2H₂O(g) → 2H₂(g) + O₂(g)

2) Mole ratios:

2 moles H₂O(g) : 2 moles H₂(g) : 2 moles O₂(g)

3) Calculate the number of moles of reactant (H₂0):

number of moles = mass in grams / molar massmolar mass of water: 18.015 g/molmass in grams of water: 42.6 gnumber of moles = 42.6 g / 18.05 g/mol = 2.36 moles H₂O

4) Set a proportion using the mole ratio  O₂ to H₂O and the actual number of moles of H₂O:

2 moles O₂ / 2 moles H₂O = x / 2.36 moles H₂Ox = 2.36 moles O₂

5) Convert 2.36 moles O₂ to grams:

mass in grams = number of moles × molar massmass = 2.36 moles × 32.00 g/mol = 75.5 g O₂

It has to be b i hope this

Ijust took the quiz. their is no coefficient needed. : )