Answer:
4.64 moles of O₂ are needed.
Explanation:
Determine the balance reaction:
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)
We verify the amount of methane at STP by the Ideal Gases Law
P . V= n . R . T
STP → 1 atm of pressure, 273K of T° (Standard conditions)
1 atm . 52L = n . 0.082 . 273K
(1 atm . 52L) / (0.082 . 273K) = n
52 / (0.082 . 273K) = n → 2.32 moles of CH₄
1 mol of methane reacts with 2 moles of oxygen
Then, 2.32 moles of methane must react with 4.64 moles of O₂ (2.32 .2) /1
