Why is that instantaneous rate of reaction does not change when a part of the reacting solution is taken out?
The instantaneous rate of reaction refers to the rate at which the concentration of a reactant or product changes at a particular moment in time. It is important to note that the rate of a reaction depends on the concentration of the reactants. When a part of the reacting solution is taken out, the overall concentration of the reactants decreases. However, the instantaneous rate of reaction does not change because it represents the rate at a specific moment and does not take into account the overall concentration of the reactants.
To understand this concept more clearly, let's consider the general equation for a chemical reaction:
aA + bB -> cC + dD
In this equation, A and B are the reactants, and C and D are the products. The coefficients (a, b, c, d) represent the stoichiometric coefficients, indicating the number of molecules or moles of each substance involved in the reaction.
The rate of reaction is determined by measuring how the concentration of a specific reactant or product changes over time. When a part of the reacting solution is taken out, the overall concentration of the reactants decreases. However, the instantaneous rate of reaction remains the same because it represents the rate at that specific moment, not the overall rate throughout the reaction.
To calculate the instantaneous rate of reaction, you need to measure the change in concentration of a reactant or product over a very short time interval. This can be done using experimental techniques like spectrophotometry, where the intensity of light passing through a reaction mixture is measured to determine the concentration.
By taking measurements at different times and calculating the rate of change in concentration, you can determine the instantaneous rate of reaction. However, it's important to remember that this rate only reflects the rate at that particular moment and does not account for changes in overall concentration that may occur due to removal of a portion of the reacting solution.