Question

Find the values for the empty cells

Brand X 3.0 5.0 33.4 0.30 33.10 0.0331 10 °C Manufacturer's name of the hydrogen peroxide solution or 2 the code number 3 Density of the hydrogen peroxide solution Percent mass H,O,(active ingredient) given on the label of the 4 solution 5 Volume of the hydrogen peroxide solution used 6 Final burette reading 7 Initial burette reading 8 Volume of gas collected 9 Liters of gas collected Temperature of the hydrogen peroxide solution after the 10 reaction 11 Temperature of the water in leveling bulb 12 Average temperature of water and solution 13 Average temperature in Kelvin 14 Barometer reading Vapor pressure at average temperature of gas (Use 15 Handbook) 16 Pressure of the gas (mmHg) 17 Pressure of the gas (atm) 18 Ideal gas law constant (R) 19 Moles of oxygen gas generated 20 Moles of H,02 21 Mass of H,02 22 Percent H,0, in the solution 23 Average percent H,0, from three trials 24 Percent difference from the label 23.5 16.75 289.9 751 °C mmHg mmHg mmHg 21.7 729.3 0.959606 0.08206 0.001335 atm L'atm/K mol moles moles 1

Answer 1

Moles of H₂O₂ = 0.00267 moles

Mass of H₂O₂ = 0.0908 g

Percent H₂O₂ in the solution = 1.82 %

Average percent H₂O₂ from three trials = 1.82 %

Percent difference from the label = 39.45 %

Explanation

The balanced chemical equation for the decomposition of H₂O₂ is :

2 H₂O₂(aq) $\rightarrow$ 2 H₂O(l) + O₂(g)

moles of O₂ = 0.001335 mol

moles H₂O₂ = (moles of O₂) * (2 moles H₂O₂ / 1 mole O₂)

moles H₂O₂ = (0.001335 mol) * (2/1)

moles H₂O₂ = 0.00267 mol

mass H₂O₂ = (moles H₂O₂) * (molar mass H₂O₂)

mass H₂O₂ = (0.00267 mol) * (34.01 g/mol)

mass H₂O₂ = 0.0908 g

percent H₂O₂ = (mass H₂O₂ / mass of solution) * 100

percent H₂O₂ = (0.0908 g / 5.0 g) * 100

percent H₂O₂ = 1.82 %