How to Balance Chemical Equations & Reactions 1 - EASY!

Summary

In this video, viewers learn how to balance chemical equations in accordance with the law of conservation of mass. The instructor explains essential concepts such as reactants, products, and the use of coefficients to balance the number of atoms on both sides of an equation. Through practical examples, the process of balancing different types of chemical reactions is broken down step by step. Emphasis is placed on understanding the role of coefficients, never changing subscripts, and the importance of balancing oxygen and other elements to ensure the equation is properly balanced. This tutorial helps demystify the balancing process, offering viewers the tools to tackle similar problems confidently.

Takeaways

• 😀 The law of conservation of mass states that the number of atoms in the reactants must equal the number of atoms in the products.
• 😀 Chemical reactions are like recipes, where reactants combine to form products, and we need to balance the equation to make sure everything adds up.
• 😀 Coefficients are used to balance chemical equations, and they represent whole number multipliers that adjust the number of atoms in the reactants and products.
• 😀 Subscripts cannot be changed when balancing equations. Only coefficients can be used to balance the atoms of each element.
• 😀 When balancing, start by identifying which elements are unbalanced and work to balance them one by one.
• 😀 Oxygen is often a key element to balance first since it can be present in multiple compounds on both sides of the equation.
• 😀 Always check that the number of atoms for each element on the reactant side equals the number of atoms on the product side after adjustments.
• 😀 The process of balancing involves multiplying elements with appropriate coefficients so that each side of the equation has the same number of atoms for every element.
• 😀 A helpful technique is to keep track of numbers like oxygen or nitrogen separately to avoid confusion while balancing.
• 😀 When faced with numbers that don't match easily (like oxygen), identify the least common multiple (LCM) to help find the right coefficients.
• 😀 It’s important to test and double-check the equation to ensure all elements are properly balanced before finalizing the equation.

Q & A

What is the Law of Conservation of Mass, and why is it important in balancing chemical equations?

The Law of Conservation of Mass states that the number of atoms in the reactants must equal the number of atoms in the products during a chemical reaction. This principle ensures that mass is neither created nor destroyed, which is fundamental in balancing chemical equations.

What are reactants and products in a chemical reaction?

Reactants are the substances that start a chemical reaction, while products are the substances that are formed as a result of the reaction. Reactants are located on the left-hand side of a chemical equation, and products are on the right-hand side.

Why can't we change the subscripts when balancing chemical equations?

Subscripts represent the number of atoms in a molecule, and changing them would alter the identity of the compounds involved. To balance the equation, we only modify the coefficients, which adjust the number of molecules, not the atoms in the molecules themselves.

What are coefficients in a chemical equation, and what is their role in balancing reactions?

Coefficients are large whole numbers placed before compounds or elements in a chemical equation. They act as multipliers, allowing us to adjust the number of molecules or atoms of each substance to balance the equation while respecting the Law of Conservation of Mass.

In the example of the iron and oxygen reaction, how was the oxygen balance achieved?

In the reaction where iron (Fe) reacts with oxygen (O₂) to form iron oxide (Fe₂O₃), the oxygen balance was achieved by placing a coefficient of 2 in front of O₂, making the number of oxygen atoms on both sides equal.

What was the issue with the sodium and oxygen reaction, and how was it corrected?

The sodium and oxygen reaction initially had an imbalance in the number of sodium atoms. The correction was made by adjusting the coefficient in front of sodium (Na) to 4, balancing the sodium atoms on both sides.

How do you approach balancing a reaction when two elements don’t have common multiples?

When elements in the reactants and products don’t have common multiples, we find the **lowest common multiple (LCM)** of the number of atoms of those elements. For example, in a reaction involving oxygen atoms with 2 and 5 atoms, the LCM of 2 and 5 is 10, which allows us to balance the equation by adjusting the coefficients appropriately.

In the example involving sulfur and carbon, how was the balance achieved?

In the sulfur and carbon example, the balance was achieved by using a coefficient of 4 for sulfur and carbon, which gave 8 sulfur atoms and 4 carbon atoms on both sides of the equation.

What is the significance of adjusting coefficients rather than subscripts in a chemical reaction?

Adjusting coefficients ensures that the equation respects the Law of Conservation of Mass by balancing the number of atoms on both sides, while maintaining the integrity of the chemical formulas. Changing subscripts would alter the chemical composition and could lead to an entirely different substance.

How can you be sure that a chemical equation is correctly balanced after adjusting the coefficients?

After adjusting the coefficients, you can check that the number of atoms for each element is equal on both sides of the equation. If the number of atoms for every element is the same on both sides, the equation is correctly balanced.