The decomposition of hydrogen peroxide is represented by the equation: 2H2O(l) + O2(g) what mass of hydrogen peroxide would be required to produce 22.4dm3 o...

The balanced chemical equation for the decomposition of hydrogen peroxide is: 2H₂O₂(l) → 2H₂O(l) + O₂(g) From the equation, it is clear that 2 moles of hydrogen peroxide will produce 1 mole of oxygen gas. Also, 1 mole of any gas at s.t.p. occupies a volume of 22.4 dm³. Therefore, to produce 22.4 dm³ of oxygen gas, we need 2 moles of hydrogen peroxide. This is because 2 moles of hydrogen peroxide will produce 1 mole of oxygen gas. Now, we can use the molar mass of hydrogen peroxide to find the mass of hydrogen peroxide needed. The molar mass of hydrogen peroxide (H₂O₂) is: 2(1.01) + 2(16.00) = 34.02 g/mol So, 2 moles of hydrogen peroxide will have a mass of: 2 mol x 34.02 g/mol = 68.04 g Therefore, 68.04 g of hydrogen peroxide is required to produce 22.4 dm³ of oxygen gas at s.t.p. Thus, the answer is (E) 68 g.