Answer:
The solutions are most likely hydrogen peroxide since it is the compound of hydrogen and oxygen that has a ratio of Hydrogen to Oxygen ratio of 1 : 1.
Note:The question is not complete.
Explanation:
The empirical formula of the two compounds are determined
Solution in beaker A:
Mass of Hydrogen = 4.425 g
Moles of hydrogen = reacting mass/molar mass = 4.425 g / 1 g/mol = 4.425 moles
Mass of oxygen = 70.575 g
Moles of oxygen = reacting mass/molar mass = 70.575 g / 16 g/mol= 4.411 moles
Mole ratio of Hydrogen to Oxygen = 4.425 : 4.411
Simplest mole ratio = 1 : 1
Therefore, empirical formula of solution in A = H₁O₁
Solution in beaker B:
Mass of Hydrogen = 7.38 g
Moles of hydrogen = reacting mass/molar mass = 7.38 g / 1 g/mol = 7.38 moles
Mass of oxygen = 117.6 g
Moles of oxygen = reacting mass/molar mass = 117.6 g / 16 g/mol= 7.35 moles
Mole ratio of Hydrogen to Oxygen = 7.38 : 7.35
Simplest mole ratio = 1 : 1
Therefore, empirical formula of solution in B = H₁O₁
The solutions in beakers A and B have the same empirical formula. Their molecular masses are not given, so their molecular formula is not certain. However, the solutions are most likely hydrogen peroxide since it is the compound of hydrogen and oxygen that has a ratio of Hydrogen to Oxygen ratio of 1 : 1.
