From a practical point of view, why would you want a reaction equilibrium to lie very far to the right?

In a chemical reaction, the term 'equilibrium' refers to the state in which the rate of the forward reaction (products forming from reactants) is equal to the rate of the reverse reaction (reactants forming from products). The position of the equilibrium determines the relative concentrations of the reactants and products at equilibrium. If the equilibrium lies far to the right, it means that most of the reactants are converted to products, and the system has a high concentration of products relative to reactants.

There are several practical reasons why having a reaction equilibrium far to the right is beneficial: 1. Higher yields: When the reaction equilibrium is far to the right, a significant amount of reactants are converted to products. This means that more of the desired product is obtained, resulting in higher yields. Higher yields are desirable in the chemical industry as it makes the process more efficient and cost-effective. 2. Less waste and environmental impact: A reaction equilibrium far to the right means less unreacted reactants remain in the system. Reactants that do not form products are considered waste, which may need to be further treated or disposed of. Therefore, reducing waste has both economic and environmental benefits. 3. Faster reaction times: A reaction driven far to the right will generally proceed at a faster rate than the same reaction driven less to the right. Faster reaction times decrease the time required to produce a desired quantity of product, which can lead to increased production and lower operating costs. 4. Simplified purification: Having a reaction equilibrium far to the right often results in fewer intermediate and by-products, likely simplifying their separation and purification. This reduces the overall complexity and cost of the post-reaction process. In conclusion, having a reaction equilibrium far to the right is generally desirable for practical purposes, as it leads to higher yields, less waste, faster reaction times, and simplified purification. These benefits contribute to cost reduction and increased efficiency in the chemical manufacturing process.