Dynamic equilibrium occurs in reversible reactions with equal forward and backward reaction rates, keeping concentrations constant. Static equilibrium involves no motion or change, as the system remains at rest. Dynamic equilibrium is ongoing, while static equilibrium is inactive.
If the temperature of the reaction is increased, the equilibrium will shift in the direction that absorbs heat (endothermic side). For water electrolysis, the decomposition of water into hydrogen and oxygen is endothermic. So the reaction rate increases. Higher temperature favours the production of H, and O, gases.
The maximum yield in a reversible reaction can be obtained by: 1. Changing temperature to favor the desired reaction (endothermic/exothermic). 2. Adjusting pressure to favour fewer gas molecules (if applicable) 3. Removing products to shift equilibrium forward
The time to attain equilibrium in a reversible reaction can be decreased by: 1. Increasing the temperature to speed up the reaction 2. Adding a catalyst to lower the activation energy 3. Increasing pressure (for gaseous reactions) or concentration of reactants
Increasing pressure has no effect on equilibrium because the number of gas molecules is the same on both sides (2 reactants vs. 2 products). The reaction remains unaffected by pressure changes.
Some reactions are irreversible because they go to completion, forming products that do not readily revert to reactants (eg., combustion). Reversible reactions occur when the products can react to form the original reactants under suitable conditions Irreversibility often happens due to energy release or product stability Reversible reactions depend on dynamic equilibrium and reaction conditions.
Combustion reactions are generally irreversible because they release a large amount of energy as heat and light The products, such as CO, and H₂O, are highly stable and do not easily convert back into reactants This makes the reverse reaction practically impossible under normal conditions.
An irreversible reaction can sometimes be made reversible by altering conditions like temperature pressure, or catalysts (eg, decomposition of calcium carbonate) A reversible reaction can become irreversible if products are removed or reaction conditions are drastically changed. Reversibility depends on the nature of the reaction and external factors.
A reaction is reversible if it reaches equilibrium, with products converting back to reactants under suitable conditions It is irreversible if it proceeds to completion, with reactants fully converting into stable products Observing energy changes and product stability helps determine reversibility.
The phase changes in water (solid to liquid, liquid to vapor) are reversible. Water can freeze into ice (solid), melt back into liquid, and evaporate into vapor, all by charging temperature or pressure. These changes can be reversed by adjusting the conditions, making them physical changes, not chemical.
To derive the reversible reaction at equilibrium in both directions, consider a general reversible The reaction: A→←B Ans The equilibrium condition is given by the principle of dynamic equilibrium, where the rate of the forward reaction is equal to the rate of the backward reaction. (a) Forward direction: In the forward direction, the reaction progresses from A to B. The rate of the forward reactions proportional to the concentration of A, and the rate constant is k, Rate (forward) = k, [A] (b) Backward direction: In the backward direction, the reaction progresses from B to A. The rate of the backward reaction is proportional to the concentration of B, and the rate constant is k Rate (backward) = k, (8) At equilibrium, the rates of both reactions are equal k₁ [A] = k [B] Rearranging this equation gives the equilibrium constant, K., for the reaction: K=[B]/[A] Thus, the equilibrium constant relates the concentrations of the products and reactants # equilibrium
As a reversible reaction progresses, the forward reaction initially occur at a fast rate due to high concentration of reactants. The backward reaction starts slowly because the product concentration is low.Over time, as the concentration of reactants decreases and the product concentration increases, the forward reaction slows, and the backward reaction speeds up. The system approaches equilibrium when the rates of the forward and backward reactions become equal. At equilibrium, the concentrations of reactants and products remain constant, although both reactions continue at the same rate.
A catalyst increases the rate of both the forward and backward reactions in a reversible reaction It provides an alternative reaction pathway with a lower activation energy, allowing the reactions to occur more quickly. However, a catalyst does not affect the position of equilibrium or the equilibrium constant It simply helps the system reach equilibrium faster without being consumed in the reaction. The concentrations of reactants and products at equilibrium remain unchanged, but equilibrium is reached more rapidly.
A reversible reaction can be forced to go to completion by 1. Removing Products: Continuously removing products shifts the equilibrium toward more product formation. 2 Adding Excess Reactant: Adding more reactant pushes the reaction toward the product side 3. Changing Temperature: Lowering temperature for exothermic reactions or increasing temperature for endothermic reactions favours the forward reaction. 4 Increasing Pressure: For gas reactions, increasing pressure shifts the equilibrium to the side with fewer gas molecules These changes help drive the reaction toward completion.
A change in temperature affects the equilibrium as follows Exothermic reaction: Increasing temperature shifts equilibrium to the left (toward reactants) Decreasing temperature shifts it to the right (toward products) Endothermic reaction: Increasing temperature shifts equilibrium to the right (toward products) Decreasing temperature shifts it to the left (toward reactants) The system adjusts to counteract the temperature change
Hydrated copper sulfate (CuSO4.5H,O) is blue because water molecules are part of its crystal Structure, giving it its colour. When heated, the water evaporates, turning the salt into anhydrous copper Sulfate (CuSO4), which is white. The loss of water changes the copper ion's coordination, causing the color to fade.
To get the maximum yield of ammonia (NH3) in the industrial synthesis process, known as the Haber Process, the following conditions are used: 1. High Pressure: A pressure of 200-300 atmospheres is applied to shift the equilibrium towards the product side (ammonia), as there are fewer gas molecules on the product side (N_{1} + 3N_{2} -> 2N*H_{1}) 2 Moderate Temperature: A temperature of 400 - 500 * C used. While lower temperatures favours ammonia production, higher temperatures increase the reaction rate. This temperature is a compromise between achieving a reasonable reaction rate and maximizing ammonia yield 3 Catalyst: Iron (Fe) is used as a catalyst, often with promoters (like potassium or aluminum oxide), to speed up the reaction without being consumed These conditions optimize the rate of reaction and maximize ammonia production while balancing efficiency and practicality.
Vast deposits of coal are available in Thar, Sindh. This coal can be used to generate electricity When coal is made to react with steam, C*O_{1} and are produced These products then react by a H_{j} reversible reaction called catalytic meth nation to yield methane
In a closed system, water exists in dynamic equilibrium between its three physical states liquid, solid, and vapor. For example, in an enclosed container at O'C, ice melts to form water, while water freezes at the same rate, maintaining balance similarly water evaporates and condenses at equal rates. Ensuring no net change in state
When dinitrogen tetroxide (N_{2}*C_{4}) kept in a sealed flask at 100 * C it dissociates into nitrogen dioxide (N*O_{1}) which is brown. Over time, the flask's colour will change from colorless to brown as more N*O_{1} forms, and equilibrium is established
Industrial production of animonie in Haber process is a very useful application of the phenomenon of chemical equilibrium. Ammonia gas leads to the formation of an important fertilizer urea the ability of ammonia gas to be converted into its liquid form easily is used to drive the reaction to completion. In this way practically 100% conversion of N2 and H2 to NH3 , is achieved.
Chemical equilibrium is the state in a reversible reaction when the rate of the forward reaction equals the rate of the reverse reaction. At this point, the concentrations of reactants and products remain constant over time, although both reactions continue to occur
The two types of equilibrium are dynamic equilibrium and static equilibrium in dynamic equilibrium, both the forward and reverse reactions occur at the same rate, while in static equilibrium, there is no movement or change, as seen in non reacting systems like a book on a table
In dynamic equilibrium, the concentrations of reactants and products do not change, as the forward and reverse reactions are occurring at the same rate The system is not static, but it appears unchanged
A reaction is at equilibrium when the concentrations of reactants and products remain constant over time and the rates of the forward and reverse reactions are equal
Le Chatelier's Principle states that if a system at equilibrium is disturbed by changing conditions (such as temperature pressure or concentration) the system will shift in a direction that counteracts the disturbance and restores equilibrium
The equilibrium constant (K) indicates the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature A high K, value means the reaction favours products, and a low K. value means it favours reactants.
Equilibrium means the rates of the forward and reverse reactions are equal, not that the concentrations of reactants and products are the same. The ratio of concentrations depends on the nature of the reaction and the equilibrium constant
A homogeneous equilibrium occurs when all the reactants and products are in the same phase, usually in a gas or liquid phase. An example is the equilibrium between gases like N₂ and H₂
A heterogeneous equilibrium occurs where reactants and products are in different phases. For example, in the equilibrium between solid calcium carbonate and its gaseous products, CaCO3 →← CaO+CO2 Solids and gases are involved
No, equilibrium can only be reached in a reversible reaction, where products can revert to reactants. A one-way reaction does not have a reverse path to establish equilibrium.
When the temperature is increased in an exothermic reaction, the equilibrium shifts toward the reactants, are the system tries to absorb the added heat by favoring the reverse reaction, which is endothermic.
Decreasing the temperature in an endothermic reaction shifts the equilibrium toward the reactants, as the system tries to release heat by favoring the exothermic reverse reaction
Increasing pressure will shift the equilibrium toward the side with fewer gas molecules. This is because the system will try to decrease the pressure by favoring the side with fewer gas molecules
Increasing pressure shifts the equilibrium toward the side with more gas molecules. The system tries to relieve the pressure by increasing the number of gas molecules.
Adding an inert gas to the system at constant pressure does not affect the equilibrium position, as inert gases do not participate in the reaction and do not change the partial pressures of the reacting gases.
Decreasing pressure in a reaction with gaseous reactants and products shifts the equilibrium toward the side with more gas molecules, as this increases the total volume, counteracting the decrease in pressure
Increasing temperature in an endothermic reaction shifts the equilibrium toward the products, as the system absorbs the added heat to favor the forward reaction, which is endothermic.
Decreasing the temperature in an exothermic reaction shifts the equilibrium toward the products, as the system releases heat to favor the exothermic forward reaction
The equilibrium constant (K) changes with temperature because it is temperature-dependent For endothermic reactions, K, increases with increasing temperature, while for exothermic reactions, K. decreases as temperature rises.
A catalyst speeds up the rate at which equilibrium is reached by lowering the activation energy. However, it does not affect the position of the equilibrium, as it accelerates both the forward and reverse reactions equally
If the concentration of a reactant is increased, the equilibrium shifts toward the products to counteract the change by consuming the added reactant and forming more products
When the concentration of a product is increased, the equilibrium shifts toward the reactants, as the system tries to use up the excess product and form more reactants.
A shift in equilibrium refers to a change in the position of equilibrium in response to a change in conditions such as temperature, pressure, or concentration. The system adjusts to minimize the effect of the disturbance
For exothermic reactions, increasing temperature shifts the equilibrium toward the reactants, while for endothermic reactions; increasing temperature shifts the equilibrium toward the products
In this reaction, the number of gas molecules is fewer on the product side (2 molecules of NH₃) compared to the reactant side (4 molecules: 1 of N2 , and 3 of H2.) Increasing pressure shifts the equilibrium toward the side with fewer gas molecules to reduce the pressure.
