## What law is used to balance equations?

Every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. Therefore, there must be the same number of atoms of each element on each side of a chemical equation.

## Do charges matter when balancing equations?

The charges of the ions in a chemical formula always add up to zero. This is because positive and negative charges attract each other. This continues to happen until the charges balance and there is no more attraction.

## How would you explain balancing an equation?

The chemical equation needs to be balanced so that it follows the law of conservation of mass. A balanced chemical equation occurs when the number of the different atoms of elements in the reactants side is equal to that of the products side. Balancing chemical equations is a process of trial and error.

## When balancing an equation you can?

When you balance an equation you can only change the coefficients (the numbers in front of molecules or atoms). Coefficients are the numbers in front of the molecule. Subscripts are the smaller numbers found after atoms. These cannot be changed when balancing chemical equations!

## How do you balance stoichiometric equations?

Balance the reaction. Start by counting the number of atoms of each element. The reaction is not balanced; the reaction has 16 reactant atoms and only 14 product atoms and does not obey the conservation of mass principle. Stoichiometric coefficients must be added to make the equation balanced.

## How do you balance chemical equations examples?

Examples of Balancing Chemical Equations

- Example 1. C5H12 + O2 —> CO2 + H2O. …
- Example 2. Zn + HCl —> ZnCl2 + H2 …
- Example 3. Ca(OH)2 + H3PO4 —> Ca3(PO4)2 + H2O. …
- Example 4. FeCl3 + NH4OH —> Fe(OH)3 + NH4Cl. …
- Example 5. S8 + F2 —> SF6 …
- Example 6. C2H6 + O2 —> CO2 + H2O. …
- Example 7. Al2(CO3)3 + H3PO4 —> AlPO4 + CO2 + H2O.

## What four guidelines are useful in balancing an equation?

General Guidelines for Balancing Simple Equations

Balance any single-element species last. Eliminate fractional coefficients (although this is not necessary). Add coefficients only; do not change the chemical formulas. There must be the same number of atoms on the left and right sides of the chemical reaction.

## What do you balance first in a chemical equation?

The first step in balancing a chemical equation is to identify your reactants and your products. Remember, your reactants are on the left side of your equation. The products are on the right side.

## How do you know if a chemical equation is balanced?

If each side of the equation has the same number of atoms of a given element, that element is balanced. If all elements are balanced, the equation is balanced.

## What three things does a balanced equation show you?

A balanced equation is an equation for a chemical reaction in which the number of atoms for each element in the reaction and the total charge is the same for both the reactants and the products. In other words, the mass and the charge are balanced on both sides of the reaction.

## What are the steps to balancing equations?

In order to balance the chemical equation, you need to make sure the number of atoms of each element on the reactant side is equal to the number of atoms of each element on the product side. In order make both sides equal, you will need to multiply the number of atoms in each element until both sides are equal.

## How do you balance an equation algebraically?

The strategy for balancing chemical equations algebraically is as follows:

- Write a different letter coefficient in front of each compound in the equation.
- Write algebraic expressions or rules for each element that equate its atoms on the LHS and RHS.

## What is the purpose of balancing equations?

Balancing Chemical equations gives us an idea about the quantity of chemical reactants that are needed for the reaction. Without balancing we just know what kind of products are obtained but with balancing chemical reactions we can also know the weight of substance produced. Because of the law of conservation of mass.