Slaked lime reacts with chlorine to give (a) \(\mathrm{CaCl}_{2}\) (b) \(\mathrm{CaO}\) (c) \(\mathrm{Ca}(\mathrm{OCl})_{2}\) (d) \(\mathrm{CaCO}_{3}\)

In chemistry, a chemical equation is a symbolic representation of a chemical reaction. It shows the reactants transforming into products, with each substance written using its chemical formula. For instance, when calcium hydroxide reacts with chlorine, the reaction can be depicted as \(\mathrm{Ca(OH)_2 + Cl_2 \rightarrow Ca(OCl)_2 + H_2O}\). It's important to balance a chemical equation to follow the Law of Conservation of Mass, which states that mass is neither created nor destroyed in a chemical reaction. The equation provided is already balanced, indicating that equal numbers of each type of atom are present on both sides of the reaction arrow.

To improve understanding, remember that the left side lists reactants, substances before the reaction, and the right side lists products, the substances formed as a result of the reaction. Place coefficients, whole numbers placed in front of chemical formulas, to balance the equation, ensuring the same quantity of each atom is reflected on both sides.

Chlorine \(\mathrm{Cl_2}\) is a highly reactive, green-yellow gas that plays a significant role in many chemical reactions. Reactivity refers to how readily a chemical species engages in chemical reactions. Chlorine is a member of the halogen group and has a strong tendency to gain electrons and form chloride ions \(\mathrm{Cl^-}\). This reactivity allows chlorine to form a variety of compounds, ranging from inorganic salts to organic chlorine compounds. In the reaction \(\mathrm{Ca(OH)_2 + Cl_2 \rightarrow Ca(OCl)_2 + H_2O}\), chlorine reacts with slaked lime to produce calcium oxychloride and water, showing chlorine's ability to react with both metals and non-metals.

When considering safety, chlorine's reactivity must be handled with caution, as it can be harmful to health and the environment, emphasizing the need for proper chemical handling protocols.

Slaked lime, scientifically known as calcium hydroxide \(\mathrm{Ca(OH)_2}\), is a white powdery substance obtained by mixing calcium oxide with water. It's slightly soluble in water, forming a suspension known as lime water, which is used in various applications including construction and wastewater treatment. Slaked lime has a basic pH and can neutralize acids, making it valuable in chemical processes requiring pH control. It's caustic and should be handled with suitable protection to avoid skin burns.

The compound's ability to react with acids and other substances like chlorine to form various compounds, including the sanitizing agent calcium oxychloride, showcases slaked lime's chemical versatility.

Calcium oxychloride \(\mathrm{Ca(OCl)_2}\), also known as bleaching powder, is formed when slaked lime (calcium hydroxide) reacts with chlorine. The chemical reaction can be summarized as \(\mathrm{Ca(OH)_2 + Cl_2 \rightarrow Ca(OCl)_2 + H_2O}\). Calcium oxychloride has disinfectant properties and is used in water treatment and as a bleach. This compound has a dual nature due to the presence of calcium, chlorine, and oxygen atoms, making it effective in various reactions. In particular, it acts as both a source of chlorine and an oxidizing agent. These properties make it useful not only for sanitizing but also in the field of organic chemistry for oxidation reactions.

Understanding the formation and uses of calcium oxychloride helps in grasping the broader implications of chemical reactions between common substances like chlorine and slaked lime.