Question

The reaction between \(\mathrm{Zn}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is an example for reaction.

Short answer

Question: Write down the balanced chemical equation for the reaction between zinc and sulfuric acid, and identify the type of reaction taking place. Answer: The balanced chemical equation for the reaction between zinc and sulfuric acid is Zn + H₂SO₄ → ZnSO₄ + H₂. This is a single displacement reaction.

Step-by-step solution

Write down the unbalanced chemical equation

The reaction between zinc and sulfuric acid can be represented by the following unbalanced equation: Zn + H₂SO₄ → ZnSO₄ + H₂

Balance the chemical equation

To balance the chemical equation, we need to ensure that the number of atoms of each element is the same on both sides of the reaction arrow. In this case, the equation is already balanced: Zn + H₂SO₄ → ZnSO₄ + H₂

Identify the type of reaction

This is an example of a single displacement reaction. In this reaction, zinc (Zn) displaces hydrogen (H) from sulfuric acid (H₂SO₄) resulting in the formation of zinc sulfate (ZnSO₄) and hydrogen gas (H₂). The balanced chemical equation for the reaction between zinc and sulfuric acid with the identification of the reaction type can be summarized as follows: Zn + H₂SO₄ → ZnSO₄ + H₂ (Single Displacement Reaction)

Key concepts

Single Displacement Reaction

Understanding how different substances interact in chemical reactions is foundational to chemistry. One such type of interaction is a single displacement reaction. In these reactions, one element trades places with another in a compound.

Picture a dance where one partner steps out, and a new partner takes their place. In chemical terms, a more reactive element will replace a less reactive one within a compound. For instance, when a metal from the activity series, such as zinc, comes into contact with the hydrogen in an acid, the zinc 'dances' into the compound's structure while 'ushering' the hydrogen out.

The equation \[ Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2 \] exemplifies this scenario. Zinc, being more reactive, displaces hydrogen from sulfuric acid to form zinc sulfate and hydrogen gas. This process not only changes the partners in the reaction but also has further implications on the reactivity series and practical applications, such as metal extractions and galvanization.

Reaction Between Zinc and Sulfuric Acid

The reaction between zinc and sulfuric acid is a classic example of a chemical reaction that is both common in laboratories and industrially significant. Zinc is a metal that reacts with sulfuric acid, a strong acid, to release hydrogen gas and form zinc sulfate—a salt.

In the laboratory, this reaction is not just a teaching tool but also a way to produce hydrogen gas on demand. The equation illustrating this reaction is: \[ Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2 \].To understand the nuances of this reaction, consider the specifics of sulfuric acid's composition, the solid state of zinc and its position in the reactivity series, and the gaseous nature of hydrogen that evolves from the reaction. This practical understanding aids students and professionals in predicting outcomes of interactions between metals and acids, and in designing experiments and industrial processes.

Chemical Equation Balancing

Chemical equation balancing is like completing a puzzle where each piece must fit precisely to maintain an overarching balance. This fundamental process ensures that the number of atoms for each element involved in the reaction remains the same before and after the chemical change, adhering to the Law of Conservation of Mass.

To balance an equation, one must systematically adjust the coefficients—the numbers placed before compounds or elements—so that the quantity of atoms is equivalent on both sides of the equation. For example: \[ Zn + H_2SO_4 \rightarrow ZnSO_4 + H_2 \].In this case, the equation is balanced as is, with one zinc atom, one sulfur atom, four oxygen atoms, and two hydrogen atoms appearing on both the reactant and product sides. It is critical for students to practice this skill, as it forms the basis for understanding stoichiometry, predicting product amounts, and scaling reactions for practical applications.

Types of Chemical Reactions

Chemistry is rich with a variety of types of chemical reactions, each with unique characteristics that define how substances transform. The main types of reactions encountered in chemistry include synthesis, decomposition, single displacement, double displacement, combustion, and acid-base reactions.

Each type of reaction is defined by a specific pattern of change.

• Synthesis: Two or more substances combine to form a single product.
• Decomposition: A compound breaks down into two or more simpler substances.
• Single Displacement: One element replaces another in a compound.
• Double Displacement: The ions of two compounds exchange places in an aqueous solution to form two new compounds.
• Combustion: A substance reacts rapidly with oxygen, often producing heat and light.
• Acid-Base: An acid reacts with a base to produce a salt and water.

Identifying the type of reaction helps chemists to predict the possible products, understand the reaction’s mechanics, and apply this knowledge to various fields such as energy production, pharmaceuticals, and environmental science.