Balance the following equations: c. CH4(𝑔)+Cl2(𝑔)⟶CCl4(𝑙)+HCl(𝑔)

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Identify the number of each type of atom on both sides of the equation. Initially, you have: Reactants: 1 C, 4 H, 2 Cl; Products: 1 C, 1 Cl, 1 H.

Notice that the carbon atoms are already balanced with 1 C on each side.

Balance the chlorine atoms. You have 2 Cl in Cl2 on the reactant side and 4 Cl in CCl4 on the product side. To balance, you need 4 Cl on the reactant side, so multiply Cl2 by 2.

Now, balance the hydrogen atoms. You have 4 H in CH4 on the reactant side and 1 H in HCl on the product side. To balance, multiply HCl by 4.

Check the balance: Reactants: 1 C, 4 H, 4 Cl; Products: 1 C, 4 Cl, 4 H. The equation is now balanced.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. To balance an equation, coefficients are adjusted in front of the chemical formulas to achieve equal atom counts.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction based on balanced equations. Understanding stoichiometry is essential for calculating yields, determining limiting reactants, and performing conversions between moles and grams.

States of Matter

The states of matter refer to the distinct forms that different phases of matter take on, primarily solid, liquid, and gas. In chemical equations, the physical state of each substance is indicated by symbols: (s) for solid, (l) for liquid, and (g) for gas. Recognizing these states is important for understanding the behavior of substances during reactions and for accurately representing the reaction conditions.

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