Using the activity series (Table 4.5), write balanced chemical equations for the following reactions. If no reaction occurs, write NR. (c) hydrobromic acid is added to tin metal

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Identify the reactants: hydrobromic acid (HBr) and tin metal (Sn).

Write the unbalanced chemical equation: \( \text{Sn} + \text{HBr} \rightarrow \text{SnBr}_2 + \text{H}_2 \).

Consult the activity series to determine if tin (Sn) can displace hydrogen (H) from hydrobromic acid (HBr).

Since tin is above hydrogen in the activity series, it can displace hydrogen, indicating a reaction will occur.

Balance the chemical equation: \( \text{Sn} + 2\text{HBr} \rightarrow \text{SnBr}_2 + \text{H}_2 \).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Activity Series

The activity series is a list of metals ranked by their ability to displace other metals from compounds in solution. More reactive metals can displace less reactive metals from their compounds, while less reactive metals cannot displace more reactive ones. This series is crucial for predicting whether a reaction will occur when a metal is introduced to an ionic solution.

Acid-Base Reactions

Acid-base reactions involve the transfer of protons (H+) between reactants. In this context, hydrobromic acid (HBr) acts as an acid, which can donate protons. Understanding how acids interact with metals is essential for determining whether a reaction will take place, particularly in the presence of a metal that may or may not react with the acid.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of the equation. This is important for accurately representing the conservation of mass in a chemical reaction. When writing equations for reactions, it is essential to balance them to reflect the stoichiometry of the reactants and products involved.

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