Final Answer:
The balanced equation for the given reaction is 2HBr + Ba(H2O)2 -> BaBr2 + 2H2O. In this reaction, hydrogen bromide (HBr) is oxidized, and barium hydroxide (Ba(H2O)2) is reduced. The oxidizing agent is barium hydroxide (Ba(H2O)2), and the reducing agent is hydrogen bromide (HBr).
Step-by-step explanation:
In the balanced chemical equation 2HBr + Ba(H2O)2 -> BaBr2 + 2H2O, we can analyze the oxidation and reduction processes. Hydrogen bromide (HBr) loses electrons to form bromine ions, indicating oxidation, while barium hydroxide (Ba(H2O)2) gains electrons to form barium ions, indicating reduction.
To balance the equation, we ensure that the same number of atoms of each element are present on both sides. The coefficients 2 in front of HBr and 2 in front of H2O balance the hydrogen and oxygen atoms. The final balanced equation is 2HBr + Ba(H2O)2 -> BaBr2 + 2H2O.
In terms of oxidation and reduction, hydrogen bromide is oxidized as it loses electrons, while barium hydroxide is reduced as it gains electrons. Therefore, hydrogen bromide is the reducing agent, facilitating the reduction process, and barium hydroxide is the oxidizing agent, facilitating the oxidation process.
In summary, the reaction involves the oxidation of hydrogen bromide and the reduction of barium hydroxide. The balanced equation reflects the conservation of mass, and the identification of the oxidizing and reducing agents helps understand the electron transfer processes occurring in the reaction.