A sample of an oxide of vanadium weighing 4.589 g was heated with hydrogen gas to form water an

step 1 Consider a couple different vanadium oxides. We're told that we have a sample of an oxide of van

A sample of an oxide of vanadium weighing 4.589 g was...

A sample of an oxide of vanadium weighing $4.589 \mathrm{~g}$ was heated with hydrogen gas to form water and another oxide of vanadium weighing $3.782 \mathrm{~g}$. The second oxide was treated further with hydrogen until only $2.573 \mathrm{~g}$ of vanadium metal remained. (a) What are the simplest formulas of the two oxides? (b) What is the total mass of water formed in the successive reactions?

A sample of an oxide of vanadium weighing $4.589 \mathrm{~g}$ was heated with hydrogen gas to form water and another oxide of vanadium weighing $3.782 \mathrm{~g}$. The second oxide was treated further with hydrogen until only $2.573 \mathrm{~g}$ of vanadium metal remained.
(a) What are the simplest formulas of the two oxides?
(b) What is the total mass of water formed in the successive reactions?

Key Concepts

Stoichiometry

Stoichiometry involves calculating the quantitative relationships between reactants and products in a chemical reaction. It relies on the mole concept, balanced equations, and proportional reasoning to determine how much of each substance is involved, ensuring that mass and atoms are conserved in the reaction.

Redox Reactions

Redox (reduction-oxidation) reactions involve the transfer of electrons between species, with one substance being oxidized and another being reduced. Understanding redox processes is key when a reducing agent, such as hydrogen, converts an oxide to a lower oxidation state or the elemental metal, while another species gains oxygen or water is formed.

Empirical Formula Determination

Empirical formula determination is the process of finding the simplest whole number ratio of atoms in a compound based on experimental data. This method uses mass measurements and mole calculations to deduce the formula from the relative amounts of different elements present.

Hydrogen Reduction of Metal Oxides

Hydrogen reduction of metal oxides is a specific type of redox reaction where hydrogen gas is used as the reducing agent to convert a metal oxide into a lower oxide or even the elemental metal while producing water. This process highlights the interplay between oxidation states and the conservation of mass.

Conservation of Mass

The conservation of mass principle asserts that mass is neither created nor destroyed in a chemical reaction. This fundamental concept is used to track changes in mass during chemical transformations, such as the loss of oxygen in metal oxides during reduction, ensuring that all mass inputs equal mass outputs.

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