2. at stp, how many liters of oxygen are required to react completely with 3.6 liters
of hydrogen to form water?
2h2(g) + o2(g)
2h20(g)

1.8 L.

Explanation:

2H₂(g) + O₂(g) → 2H₂O(g),

It is clear that 2.0 moles of H₂ react with 1.0 mole of O₂ to produce 2.0 moles of H₂O.

It is known that at STP: every 1.0 mol of any gas occupies 22.4 L.

using cross multiplication:

1.0 mol of H₂ represents → 22.4 L.

??? mol of H₂ represents → 3.6 L.

∴ 3.6 L of H₂ represents = (1.0 mol)(3.6 L)/(22.4 L) = 0.1607 mol.

Using cross multiplication:

2.0 mol of H₂ react completely with → 1.0 mol of O₂, from stichiometry.

0.1607 mol of H₂ react completely with → ??? mol of O₂.

∴ The no. of moles of O₂ = (1.0 mol)(0.1607 mol)/(2.0 mol) = 0.08036 mol.

1.0 mol of O₂ represents → 22.4 L, at STP.

0.08036 mol of O₂ represents → ??? L.

∴ The no. of liters of O₂ will be produced = (0.08036 mol)(22.4 L)/(1.0 mol) = 1.8 L.

where is the following

explanation: