What mass of water is produced when 10.0 L of oxygen react completely in the following equation? 2 H₂(g)+ O₂(g)$\rarr$ 2 H₂O(l)

Question

Quizplus · Accepted Answer

From the balanced chemical equation, we can see that 2 moles of H2SO4 react with 1 mole of O2 to produce 2 moles of H2SO4O (water).
Molar volume of any gas at STP (standard temperature and pressure) is 22.4 L/mol.
Hence, the number of moles of O2 in 10 L of oxygen is:
n = V/Vm = 10/22.4 = 0.4464 moles
Therefore, the number of moles of water produced in the reaction is:
n(H2O) = 2n(O2) = 0.8928 moles

The molar mass of water is 18 g/mol.
Therefore, the mass of water produced is:
m(H2O) = n(H2O) x MM(H2O) = 0.8928 x 18 = 16.07 g ≈ 16.1 g

Thus, the best choice is B) 16.1 g as it is the calculated mass of water produced.

What Mass of Water Is Produced When 10 →\rarr→ 2 H2O(l) A)4

What Mass of Water Is Produced When 10 $\rarr$ 2 H₂O(l)
A)4