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Chapter 12: Problem 1

State the law of conservation of mass, and give an example.

Short Answer

Expert verified
Mass is conserved in chemical reactions; total mass of reactants equals total mass of products, as shown in \( 2H_2 + O_2 \rightarrow 2H_2O \).

Step by step solution

01

Understanding the Concept

The law of conservation of mass states that mass cannot be created or destroyed in a closed system through ordinary chemical reactions or physical changes. Instead, mass can only be transformed from one form to another.
02

Identify a Real-world Example

One of the most common examples of the law of conservation of mass is in a chemical reaction, such as the reaction of hydrogen and oxygen to form water.
03

Describe the Example

Consider the balanced chemical equation for the formation of water: \( 2H_2 + O_2 \rightarrow 2H_2O \). In this reaction, two molecules of hydrogen gas react with one molecule of oxygen gas to form two molecules of water. The total mass of the reactants (hydrogen and oxygen) equals the total mass of the products (water). This illustrates that mass is conserved.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Chemical Reactions
Chemical reactions are processes where substances, known as reactants, transform into new substances, referred to as products. During this transformation, chemical bonds between atoms in the reactants are broken and new bonds are formed in the products.
A notable example is the reaction between hydrogen and oxygen to form water. This can be represented by the chemical equation:
  • \( 2H_2 + O_2 \rightarrow 2H_2O \)
In this equation:
  • Two molecules of hydrogen (\(2H_2\)) combine with one molecule of oxygen (\(O_2\)).
  • The reaction produces two molecules of water (\(2H_2O\)).
Importantly, the number and type of atoms are the same on both sides of the equation, satisfying the law of conservation of mass.
Physical Changes
Physical changes involve the alteration of the state or appearance of a substance without changing its chemical composition. Think of ice melting into water. Here, the water molecules stay the same but change their state from solid ice to liquid water.
Physical changes can be characterized by:
  • Changes in state (solid, liquid, gas)
  • Alterations in form (size, shape)
  • No new substances being formed
Unlike chemical reactions, the identity of the substance does not change. Hence, just like in chemical reactions, the mass remains conserved throughout the change.
Closed System
A closed system fully encapsulates all components involved in a process, ensuring no exchange of matter with the outside environment. This concept is vital when discussing the conservation of mass because it ensures that all reactants and products remain contained.
In a closed system:
  • No matter enters or leaves the system.
  • Mass is not lost or gained from the surroundings.
  • It provides an isolated environment to observe the true conservation of mass during reactions or changes.
Such systems can be found in laboratory experiments where reactions are sealed in containers or vessels that do not allow substances to escape.
Mass Transformation
The principle of mass transformation is rooted in the idea that during any chemical reaction or physical change, the total mass remains constant. This ties directly to the law of conservation of mass, which asserts that mass is neither created nor destroyed.
Mass transformation involves:
  • Transitioning of reactants to products while maintaining total mass.
  • Reallocation of atoms to form new chemical bonds.
  • Ensuring the mass before and after the transformation is equal.
Consider again the reaction forming water: although hydrogen and oxygen gases are transformed into water, the total mass of the system remains unchanged. This principle is a fundamental aspect of chemistry that underscores the predictability and balance of chemical processes.

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Most popular questions from this chapter

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