Question

I have two beakers (A & B) containing clear liquids. The first one (A) holds 75g and after being analyzed proves to contain 4.425g of hydrogen and 70.575g of oxygen. The second beaker (B) holds 125g and analysis shows that it is composed of 7.38g of hydrogen and 117.6g of oxygen.

Answer 1

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.

Step-by-step 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.