Hydrogen peroxide decomposes into oxygen and water. What mass of hydrogen peroxide is required to produce 1L of oxygen?
Correct answer: D. 3 g
- A. 1.5 g
- B. 1 g
- C. 2 g
- D. 3 g
Explanation
H2O2 decomposes into O2 and H2O by the following reaction: 22.4 dm3 of O2 = 1 mole of O2 1 dm3 of O2 = 1/22.4 moles of O2 According to the equation; Production of 1 mole of O2 requires 2 moles of H2O2. So 1/22.4 moles of O2 require = (2/22.4) = 1/11.2 moles of H2O2 1 mole of H2O2 = 34 g 1/11.2 moles of H2O2 = 34/11.2 g = 3g Thus 3g of H2O2 must be decomposed to produce 1 dm3 or 1 L of O2.
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About Fundamental Concepts of Chemistry
Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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