FreeNotes
To shift equilibrium in the forward direction, conditions must be adjusted to favor the products. This can include increasing the temperature (for exothermic reactions), increasing the concentration of reactants, or decreasing the concentration of products. In the case of gaseous reactions, increasing the pressure can shift the equilibrium toward the side with fewer gas molecules. … Read more
To drive a reversible reaction to completion, you can apply changes that shift the equilibrium toward the products. This can include removing products as they form (e.g., by distillation or precipitation), adding more reactants to increase their concentration, or altering conditions such as temperature or pressure to favor the forward reaction. In some cases, the … Read more
Some reactions are irreversible due to the energy changes involved and the stability of the products. For example, combustion reactions release a large amount of energy, which results in the complete breakdown of reactants into simpler products that are very stable and cannot easily revert back to the original reactants. Other reactions, such as the … Read more
Pressure affects equilibria involving gases. According to Le Chatelier’s Principle, if the pressure is increased, the equilibrium will shift in the direction that produces fewer gas molecules to counteract the pressure change. Conversely, decreasing the pressure shifts the equilibrium toward the side with more gas molecules. In reactions that do not involve gases or involve … Read more
In some cases, it is possible to make an irreversible reaction reversible by altering the reaction conditions. For instance, by applying high temperatures or pressures, or by changing the medium in which the reaction occurs, you may be able to reverse the direction of the reaction. However, this is not always possible, as many reactions, … Read more
To increase the maximum yield of a reversible reaction, you can adjust the conditions in accordance with Le Chatelier’s Principle. You can increase the concentration of reactants or decrease the concentration of products to shift the equilibrium toward the product side. Increasing the pressure (for reactions involving gases) or lowering the temperature (for exothermic reactions) … Read more
Hydrated copper sulfate (CuSO₄·5H₂O) is blue in color due to the presence of water molecules in its crystalline structure. The water molecules form a complex with copper ions, which gives the crystal its characteristic blue hue. When heated, the water evaporates, and the salt loses its blue color. This is because the removal of water … Read more
As a system approaches equilibrium, the rates of the forward and backward reactions change. Initially, the rate of the forward reaction is higher because reactants are being converted into products. Over time, as the concentration of the products increases and the concentration of the reactants decreases, the rate of the forward reaction slows down. Simultaneously, … Read more
Hybridization is the process in which atomic orbitals mix to form new hybrid orbitals, which are used to form covalent bonds in molecules. This concept helps explain the geometry of molecules in a more accurate way than just considering the atomic orbitals of individual atoms. sp Hybridization: Occurs when one s orbital and one p … Read more
Ionic Bond: Formation: Occurs when electrons are transferred from one atom to another, resulting in the formation of positive and negative ions. Example: Sodium chloride (NaCl) is formed when sodium donates an electron to chlorine. Properties: High melting and boiling points, electrical conductivity when dissolved in water or molten, usually soluble in water. Covalent Bond: … Read more