3.10
Chemical Equations
Chemical reactions involve chemical transformations of one or more substances into different materials. A reaction is conventionally represented using a chemical equation, which utilizes chemical formulas to represent atoms, molecules, or compounds involved.
The substances present at the start of a reaction and consumed during the process are called reactants. Reactants are specified on the left side of the equation. The substances formed during the reaction are called products and are indicated on the right side of the equation.
An arrow separating the reactants and products shows the direction of the reaction. The different states of matter are depicted using parenthesized abbreviations.
A chemical reaction observes the law of conservation of mass, where the total masses of all participating elements are conserved. Therefore, the cumulative number of atoms of each element will match in both the reactants and products.
Chemical equations are balanced using numerical coefficients to reflect the actual number of atoms involved in the reaction. It is important to only change the numerical coefficients and not numerical subscripts that define the identity of a compound while balancing any chemical equation.
General guidelines help illustrate and adjust a chemical equation efficiently.
For example, the combustion of liquid benzoic acid, forming gaseous carbon dioxide and water is represented initially using a skeletal chemical equation. The atoms are balanced next by first adjusting those within the compounds, followed by the atoms of free elements.
The inclusion of coefficients seven and three before the formulas for carbon dioxide and water balances the carbon and hydrogen atoms. A fractional coefficient of 15/2 adjusts the oxygen atoms.
Fractional coefficients are converted to whole numbers by multiplying the complete equation by the denominator. The collective number of atoms of each element equals on both sides in a balanced equation.
In chemical equations representing reactions involving ionic compounds, the cations are balanced first, followed by the anions. Polyatomic ions are always balanced as a unit.
For example, aqueous aluminum sulfate reacts with aqueous calcium hydroxide forming solid aluminum hydroxide and solid calcium sulfate. Using a skeletal equation, the cations of aluminum and calcium are balanced, followed by the anions of polyatomic hydroxide and sulfate ions. Lastly, the coefficients are adjusted to get an overall balanced equation.
Chemical equations represent the identities and relative quantities of substances involved in a chemical reaction. The substances undergoing reaction are called reactants, and their formulas are placed on the left side of the equation. The substances generated by the reaction are called products, and their formulas are placed on the right side of the equation. Plus signs (+) separate individual reactant and product formulas, and an arrow (→) separates the reactant and product (left and right) sides of the equation. The relative numbers of reactant and product species are represented by numerical coefficients, placed immediately to the left of each formula. A coefficient of 1 is typically not usually shown. The smallest possible whole-number coefficients are commonly used in a chemical equation, and they are interpreted as ratios. For example, methane and oxygen react to yield carbon dioxide and water in a 1:2:1:2 ratio.
The ratio indicates that the smallest possible coefficients of methane, oxygen, carbon dioxide, and water are 1, 2, 1, and 2, respectively. The coefficients may be interpreted with regard to any amount (number) unit, and so this equation may be correctly read in many ways, including:
i. One methane molecule and two oxygen molecules react to yield one carbon dioxide molecule and two water molecules.
ii. One mole of methane molecules and 2 moles of oxygen molecules react to yield 1 mole of carbon dioxide molecules and 2 moles of water molecules.
The physical states of reactants and products in chemical equations very often are indicated with a parenthetical abbreviation following the formulas. Standard abbreviations include ‘s’ for solids, ‘l’ for liquids, ‘g’ for gases, and ‘aq’ for substances dissolved in water.
Balancing equations
In a balanced equation, the numbers of atoms for each element involved in the reaction are the same on the reactant and product sides, thereby satisfying the law of conservation of matter. A balanced equation can be confirmed by adding the numbers of atoms on either side of the arrow and comparing these sums to ensure they are equal. Note that the number of atoms for a given element is calculated by multiplying the coefficient of any formula containing that element by the element’s subscript in the formula. If an element appears in more than one formula on a given side of the equation, the number of atoms represented in each must be computed and then added together.
To balance the equation, the coefficients of the equation may be changed as needed. It is sometimes convenient to use fractions instead of integers as intermediate coefficients in the process of balancing a chemical equation. When balance is achieved, all the equation’s coefficients may then be multiplied by a whole number to convert the fractional coefficients to integers without upsetting the atom balance.
For example, the reaction of ethane (C2H6) with oxygen yields water and carbon dioxide, which can be represented by the following unbalanced equation:
The unbalanced equation contains:
| Atoms | Reactant | Product | Balanced? |
| C | 2 | 1 | No |
| H | 6 | 2 | No |
| O | 2 | 3 | No |
To balance the number of carbon atoms and hydrogen atoms, multiply CO2 by the coefficient 2 and multiply H2O by the coefficient 3, respectively. This changes the total number of oxygen atoms on the product to 7. To balance the number of oxygen atoms, multiply oxygen by the fractional coefficient 7/2. This initial balancing of the carbon, hydrogen, and oxygen atoms by changing the coefficients for reactants and products, gives the provisionally balanced equation:
A conventional balanced equation with integer-only coefficients is derived by multiplying each coefficient by 2, to generate the equation:
This text is adapted from Openstax, Chemistry 2e, Section 4.1: Writing and Balancing Chemical Equations.
Chemical reactions involve chemical transformations of one or more substances into different materials. A reaction is conventionally represented using a chemical equation, which utilizes chemical formulas to represent atoms, molecules, or compounds involved.
The substances present at the start of a reaction and consumed during the process are called reactants. Reactants are specified on the left side of the equation. The substances formed during the reaction are called products and are indicated on the right side of the equation.
An arrow separating the reactants and products shows the direction of the reaction. The different states of matter are depicted using parenthesized abbreviations.
A chemical reaction observes the law of conservation of mass, where the total masses of all participating elements are conserved. Therefore, the cumulative number of atoms of each element will match in both the reactants and products.
Chemical equations are balanced using numerical coefficients to reflect the actual number of atoms involved in the reaction. It is important to only change the numerical coefficients and not numerical subscripts that define the identity of a compound while balancing any chemical equation.
General guidelines help illustrate and adjust a chemical equation efficiently.
For example, the combustion of liquid benzoic acid, forming gaseous carbon dioxide and water is represented initially using a skeletal chemical equation. The atoms are balanced next by first adjusting those within the compounds, followed by the atoms of free elements.
The inclusion of coefficients seven and three before the formulas for carbon dioxide and water balances the carbon and hydrogen atoms. A fractional coefficient of 15/2 adjusts the oxygen atoms.
Fractional coefficients are converted to whole numbers by multiplying the complete equation by the denominator. The collective number of atoms of each element equals on both sides in a balanced equation.
In chemical equations representing reactions involving ionic compounds, the cations are balanced first, followed by the anions. Polyatomic ions are always balanced as a unit.
For example, aqueous aluminum sulfate reacts with aqueous calcium hydroxide forming solid aluminum hydroxide and solid calcium sulfate. Using a skeletal equation, the cations of aluminum and calcium are balanced, followed by the anions of polyatomic hydroxide and sulfate ions. Lastly, the coefficients are adjusted to get an overall balanced equation.
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