(c) As a reaction proceeds, does the instantaneous reaction rate increase or decrease?

Verified step by step guidance

1. 1. The instantaneous reaction rate refers to the rate of reaction at a particular moment in time. It is the rate at which reactants are consumed or products are formed at that specific instant.
2. 2. As a reaction proceeds, the concentration of the reactants decreases because they are being used up to form products. This is a fundamental principle of chemical reactions.
3. 3. The rate of a reaction is often proportional to the concentration of the reactants. This relationship is described by the rate law, which is an equation that relates the reaction rate to the concentrations of the reactants.
4. 4. Therefore, as the reaction proceeds and the concentration of the reactants decreases, the instantaneous reaction rate also decreases.
5. 5. In conclusion, the instantaneous reaction rate generally decreases as a reaction proceeds, unless the reaction is zero order, in which case the rate is constant and does not depend on the concentration of the reactants.

Key Concepts

Reaction Rate

The reaction rate is a measure of how quickly reactants are converted into products in a chemical reaction. It is typically expressed as the change in concentration of a reactant or product per unit time. Understanding the factors that influence reaction rates, such as concentration, temperature, and catalysts, is essential for analyzing how these rates change over the course of a reaction.

Instantaneous Rate

The instantaneous rate of a reaction refers to the rate at a specific moment in time, rather than over an interval. It can be determined by taking the slope of the tangent line to the concentration vs. time curve at that point. This concept is crucial for understanding how the rate of reaction evolves as reactants are consumed and products are formed.

Reaction Mechanism

A reaction mechanism is a detailed description of the step-by-step process by which reactants are transformed into products. It includes the sequence of elementary steps, intermediates, and transition states involved. The mechanism can influence how the instantaneous reaction rate changes, as different steps may have varying rates and can be affected by factors like concentration and temperature.