Question

Although silver is not easily attacked by acids (and for that reason it has been used to make jewelry and household items), it will dissolve in concentrated nitric acid, producing brown NO gas and leaving a solution of silver nitrate in water. Write the unbalanced chemical equation for this process.

Short answer

The balanced chemical equation for the reaction between silver (Ag) and concentrated nitric acid (HNO₃), which produces silver nitrate (AgNO₃) and brown NO gas, is: \[ 3Ag + 4HNO_3 → 3AgNO_3 + 2NO + 2H_2O \]

Step-by-step solution

Identify reactants and products

The reactants given are silver (Ag) and concentrated nitric acid (HNO₃). The products mentioned are brown NO gas and a solution of silver nitrate (AgNO₃) in water.

Write the unbalanced chemical equation

Now, we will write down the unbalanced chemical equation based on the given reactants and products: \[ Ag + HNO_3 → AgNO_3 + NO \]

Balance the chemical equation

In order to balance the chemical equation, we will adjust the coefficients (numbers written in front of molecules) properly so that the number of atoms for every element on the reactant side is equal to the number of atoms for the corresponding element on the product side. The balanced chemical equation for the reaction between silver and concentrated nitric acid is: \[ 3Ag + 4HNO_3 → 3AgNO_3 + 2NO + 2H_2O \] Here, the number of atoms for every element on the reactant and product sides is equal (3 Ag, 12 H, 12 N, and 12 O atoms).

Key concepts

Balancing Chemical Equations

Balancing chemical equations is a crucial skill in chemistry that ensures the law of conservation of mass is maintained. When a chemical reaction occurs, atoms are not created or destroyed but rearranged. This means the number of atoms of each element in the reactants must equal the number in the products.

To balance an equation, you adjust the coefficients, which are the numbers placed before the substances in the reaction. Coefficients change the amount of substance but not its identity. Start by writing down the unbalanced equation, then systematically adjust the coefficients to ensure each element has the same number of atoms on both sides. It's like solving a puzzle where the pieces need to fit perfectly.

For example, in our exercise with silver and nitric acid, the unbalanced equation was: \[ Ag + HNO_3 → AgNO_3 + NO \]Balancing it resulted in: \[ 3Ag + 4HNO_3 → 3AgNO_3 + 2NO + 2H_2O \]

This ensures that all elements have equal counts on both sides.

Silver Nitrate

Silver nitrate (AgNO₃) is a compound formed when silver reacts with nitric acid. It is commonly used in various applications, including photography, medicine, and chemical synthesis.

In this reaction, silver initially reacts with concentrated nitric acid, resulting in the formation of silver nitrate and other by-products like NO gas and water. The chemical formula of silver nitrate is AgNO₃, where 'Ag' represents silver, 'N' represents nitrogen, and 'O' stands for oxygen.

• Silver nitrate is water-soluble, meaning it can dissolve in water, forming a clear solution.
• It has antibacterial properties, making it useful for medical creams and wound dressings.
• In photography, it acts as a light-sensitive material.

By understanding the properties and uses of silver nitrate, one can appreciate its significance in various fields.

Nitric Acid

Nitric acid (HNO₃) is a strong, highly corrosive acid known for its ability to dissolve metals such as silver. It's a vital reagent in both laboratory and industrial settings.

In our chemical reaction, nitric acid reacts with silver, forming silver nitrate, NO gas, and water. The formula HNO₃ consists of hydrogen, nitrogen, and oxygen. Here are some important aspects of nitric acid:

• It is a key component in the production of fertilizers, explosives, and other chemicals.
• Nitric acid can produce toxic fumes, so it needs to be handled with care.
• Its ability to oxidize makes it useful in metal etching and refining processes.

Understanding its role and properties clarifies why it reacts the way it does with silver.

NO Gas

Nitric oxide (NO) is a colorless gas formed as a by-product in various chemical reactions, including the reaction between silver and nitric acid. Despite its simple composition, consisting of just one nitrogen atom and one oxygen atom, NO plays significant roles in both nature and industry.

In the reaction described, NO appears as a brown gas, a characteristic often seen when it exits the reaction environment and interacts with the air. Here are a few key points about NO gas:

• It's important in industrial processes and the synthesis of other chemicals.
• NO can contribute to air pollution, being one of the gases involved in acid rain formation.
• In biological systems, NO plays a role in signaling pathways, helping to regulate processes such as blood flow.

Recognizing its formation in reactions helps understand larger environmental and industrial implications.

Reactants and Products

In any chemical reaction, we have reactants and products. Understanding these terms is essential for writing and balancing chemical equations.

Reactants are substances initially present, undergoing change during the reaction. Products are what you get after the reaction has occurred. In the reaction between silver and concentrated nitric acid, the identified reactants were:

• Silver (Ag)
• Nitric Acid (HNO₃)

And the resulting products were:

• Silver Nitrate (AgNO₃)
• Nitric Oxide (NO)
• Water (H₂O)

Recognizing reactants and products involves noting what substances start the reaction and what substances form after. This foundational knowledge enables you to write equations accurately and is crucial in the understanding of chemical processes.