Question

When copper(II) oxide is boiled in an aqueous solution of sulfuric acid, a strikingly blue solution of copper(II) sulfate forms along with additional water. Write the unbalanced chemical equation for this reaction.

Short answer

The balanced chemical equation for the reaction between copper(II) oxide and sulfuric acid is: CuO + H₂SO₄ → CuSO₄ + H₂O

Step-by-step solution

Write the unbalanced chemical equation

For this step, write down the reactants and products. As mentioned above, they are copper(II) oxide (CuO), sulfuric acid (H₂SO₄), copper(II) sulfate (CuSO₄) and water (H₂O). The unbalanced equation is: CuO + H₂SO₄ → CuSO₄ + H₂O

Count the atoms on both sides of the equation

This step helps us to identify which elements need to be balanced. Counting the atoms on both sides, we get: Reactants: Copper (Cu) → 1 Oxygen (O) → 2 Hydrogen (H) → 2 Sulfur (S) → 1 Products: Copper (Cu) → 1 Oxygen (O) → 5 Hydrogen (H) → 2 Sulfur (S) → 1 Notice that we need to balance the Oxygen atoms.

Balance the atoms

To balance the atoms on both sides, we can change the coefficients (the numbers in front of the elements/compounds) but not the subscripts. To balance the Oxygen atoms, we don’t need to modify any coefficients because the total number of Oxygen atoms on both sides is already equal. Reactants: Copper (Cu) → 1 Oxygen (O) → 2 Hydrogen (H) → 2 Sulfur (S) → 1 Products: Copper (Cu) → 1 Oxygen (O) → 5 Hydrogen (H) → 2 Sulfur (S) → 1 Now, all the atoms on both sides are balanced. The final balanced equation is: CuO + H₂SO₄ → CuSO₄ + H₂O

Key concepts

Copper(II) Oxide

Copper(II) Oxide, with the chemical formula \(CuO\), is a black solid compound. It is made up of copper and oxygen. This compound is often used in reactions to form other copper compounds, as it acts as an intermediate substance in many industrial processes.
When copper(II) oxide comes into contact with an acid, like sulfuric acid, it undergoes a chemical reaction where it can be converted into a different copper-based compound. In this case, it transforms into copper(II) sulfate (\(CuSO_4\)). Understanding the role of copper(II) oxide is crucial, as it typically serves as one a reactant (starting material) in chemical reactions.

Sulfuric Acid

Sulfuric acid is a highly reactive substance with the chemical formula \(H_2SO_4\). It is a dense, colorless, and oily liquid that is widely used in a variety of processes. Its capability as a strong acid allows it to participate in reactions that result in the formation of salts and water, a type of reaction known as neutralization.
In the reaction with copper(II) oxide, sulfuric acid donates protons and reacts to form copper(II) sulfate. As one of the reactants, sulfuric acid provides the sulfur and some of the oxygen needed to create the chemical bonds found in the copper(II) sulfate product.
Sulfuric acid is essential in industries for processes such as fertilizer production, oil refining, and wastewater processing, underlining its importance beyond just one chemical reaction.

Copper(II) Sulfate

Copper(II) sulfate, denoted by \(CuSO_4\), is a bright blue compound produced in the reaction between copper(II) oxide and sulfuric acid. This compound is notable for its vivid color and forms part of many other industrial and laboratory applications.
Its formation is key in the reaction as it signifies the copper(II) oxide has successfully reacted with sulfuric acid. Copper(II) sulfate serves various purposes, from fungicides and herbicides in agriculture to electrolyte solutions in electroplating and batteries.
Knowing how to produce copper(II) sulfate effectively by understanding its chemical reactions can be quite beneficial, as it has an array of applications that touch everyday life and several industrial processes.

Balancing Chemical Equations

Balancing chemical equations is a fundamental skill in chemistry that ensures the number of atoms for each element is equal on both sides of the equation. An equation is balanced by adjusting the coefficients (the numbers in front of substances) but not the subscripts (numbers within the chemical formulas).
In our original exercise, the equation \(CuO + H_2SO_4 \rightarrow CuSO_4 + H_2O\) needed balancing. Despite initially seeming unbalanced, with proper counting and verification, no coefficient changes were necessary, as each type of atom was already present in equal amounts on both sides.
The main purpose of balancing equations is to satisfy the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. This principle maintains that all atoms present in the reactants must be accounted for in the products, ensuring the equation accurately represents the chemical reaction.