Answer:
0.12 g of O2.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is given below:
H2O2 —> H2 + O2
Next, we shall determine the mass of H2O2 that decomposed and the mass of O2 produced from the balanced equation. This is illustrated below:
Molar mass of H2O2 = (2×1) + (16×2)
= 2 + 32
= 34 g/mol
Mass of H2O2 from the balanced equation = 1 × 34 = 34 g.
Molar mass of O2 = 16×2 = 32 g/mol
Mass of O2 from the balanced equation = 1 × 32 = 32 g
Summary:
From the balanced equation above,
34 g of H2O2 decomposed to produce 32 g of O2.
Finally, we shall determine the mass of O2 produced from the decomposition of 0.128 g of H2O2. This can be obtained as follow:
From the balanced equation above,
34 g of H2O2 decomposed to produce 32 g of O2.
Therefore, 0.128 g of H2O2 will decompose to produce = (0.128×32)/34 = 0.12 g of O2.
Therefore, 0.12 g of O2 was produced.
