Write balanced chemical equations to correspond to each of the following descriptions: (d) When solid mercury(II) nitrate is heated, it decomposes to form solid mercury(II) oxide, gaseous nitrogen dioxide, and oxygen. (e) Copper metal reacts with hot concentrated sulfuric acid solution to form aqueous copper(II) sulfate, sulfur dioxide gas, and water.

Verified step by step guidance

1. Identify the chemical formula for each compound: Mercury(II) nitrate is \( \text{Hg(NO}_3\text{)}_2 \), mercury(II) oxide is \( \text{HgO} \), nitrogen dioxide is \( \text{NO}_2 \), and oxygen is \( \text{O}_2 \).
2. Write the unbalanced chemical equation for the decomposition reaction: \( \text{Hg(NO}_3\text{)}_2 (s) \rightarrow \text{HgO} (s) + \text{NO}_2 (g) + \text{O}_2 (g) \).
3. Balance the equation by adjusting coefficients to ensure the same number of each type of atom on both sides of the equation.
4. Start by balancing the mercury atoms: There is 1 mercury atom on both sides, so they are balanced.
5. Next, balance the nitrogen and oxygen atoms by adjusting the coefficients of \( \text{NO}_2 \) and \( \text{O}_2 \) to ensure the total number of nitrogen and oxygen atoms are equal on both sides.

Key Concepts

Decomposition Reactions

Decomposition reactions occur when a single compound breaks down into two or more simpler products. In this case, solid mercury(II) nitrate decomposes upon heating, which is a common characteristic of many metal nitrates. Understanding this type of reaction is essential for predicting the products formed during the heating process.

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 based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Proper balancing is crucial for accurately representing the reaction and its stoichiometry.

Products of Thermal Decomposition

The thermal decomposition of certain compounds can yield specific products, often including oxides, gases, or other simpler compounds. In the case of mercury(II) nitrate, heating leads to the formation of mercury(II) oxide, nitrogen dioxide, and oxygen. Recognizing the typical products of thermal decomposition helps in predicting the outcomes of similar reactions.