\r\n \r\n Introduction\r\n
\r\n \r\n A chemical equation is a way of representing a chemical reaction using symbols (to represent chemical entities) and numeric coefficients (to represent stoichiometry) of the various chemical entities involved in the reaction.\r\n \r\n \r\n Reactants & Products\r\n
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\r\n \r\n For example, the chemical equation representing synthesis of ammonia is given as: $$ N_2 + 3H_2 \\rightarrow 2NH_3$$\r\n In this reaction, \\(N_2\\)(Nitrogen) and \\(H_2\\) (Hydrogen) are the reactants, and \\(NH_3\\) (Ammonia) is the product. During the reaction, 1 molecule of \\(N_2\\) reacts with 3 molecules of \\(H_2\\) to produce 2 molecules of \\(NH_3\\).\r\n \r\n It is a common practice to use the smallest whole numbers as coefficients in a chemical equation — as shown in this example.\r\n \r\n \r\n \r\n \r\n Balancing a Chemical Equation\r\n
\r\n \r\n In a chemical reaction, matter is neither created nor destroyed, therefore every chemical reaction should be consistent with the law of conservation of mass.
\r\n This requires that the mass of every chemical species involved in the reaction should remain the same before and after the reaction. When a chemical equation satisfies this condition, the equation is said to be \"balanced,\" otherwise, the equation is said to be \"unbalanced.\"\r\n \r\n Let's take the example of the reaction describing the synthesis of water molecules from a combination of hydrogen and oxygen molecules.\r\n $$ H_2 + O_2 \\rightarrow H_2 O$$ Let's check if this equation is balanced or unbalanced.\r\n
On the reactant side (shown on the left) — we have 2 Hydrogen atoms and 2 Oxygen atoms.\r\n \r\n On the product side (shown on the right) — we have 2 Hydrogen atoms, however, only 1 Oxygen atom.\r\n \r\n So, clearly the equation is unbalanced.\r\n \r\n Let's multiply the right side by a factor of 2 so that we now have 2 Oxygen atoms on each side. $$ H_2 + O_2 \\rightarrow 2 H_2 O$$\r\n However, now we have 4 Hydrogen atoms on the product side and only 2 of those in the reactant side. So, in order to balance the number of Hydrogen atoms, we multiply \\(H_2 \\) on the reactant side with 2, and that makes the equation balanced.\r\n $$ 2 H_2 + O_2 \\rightarrow 2 H_2 O$$.\r\n \r\n\r\n \r\n \r\n
\r\n \r\n Lavoisier discovered the law of conservation of mass, which states that the mass remains conserved during a chemical reaction. This principle forms the basis for balancing chemical equations.\r\n
\r\n \r\n \r\n \r\n \r\n Lesson Plan \r\n
\r\n \r\n This chapter on balancing chemical equations contains three interactive lessons. Each lesson includes a visually interactive exercise that offers students a uniquely engaging and effective learning experience.\r\n \r\n Lesson 1 | Combustion of Hydrocarbons
\r\n In this lesson, you will learn to balance a chemical equation representing combustion of a hydrocarbon (such as Methane, Ethane, Propane or Butane).\r\n \r\n Lesson 2 | Chlorination of Metals
\r\n This lesson includes visually interactive aids on balancing chemical equations describing chlorination of metals.\r\n \r\n Lesson 3 | Oxidation of Metals
\r\n This lesson includes visually interactive aids on balancing chemical equations representing oxidation of metals.\r\n
\r\n\r\n \r\n Let's get started\r\n
\r\n \r\n Check out our library of meticulously crafted lessons on balancing chemical equations. These specially designed lessons use visuo-spatiality and interactivity to help students improve engagement and retain concepts.\r\n \r\n \r\n \r\n \r\n \r\n \r\n \r\n \r\n
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