Rate of reaction curve for equilibrium can be like: `[r_(f)=` forward rate, `r_(b) =` backward rate]

Explanation

To analyze the rate of reaction curve for equilibrium involving the forward rate (Rf) and backward rate (Rb), we can follow these steps:

### Step-by-Step Solution:

1. **Understanding the Reaction**:
- Consider a general reaction: A + B ⇌ C + D.
- In this reaction, A and B are the reactants, and C and D are the products.

2. **Initial Conditions**:
- At time \( t = 0 \), the concentrations of A and B are at their maximum, while the concentrations of C and D are zero. This is because no reaction has occurred yet.

3. **Reaction Progression**:
- As time progresses, the reaction begins to proceed forward, meaning A and B are consumed to form C and D.
- Consequently, the concentration of A and B decreases, while the concentration of C and D increases.

4. **Rate Changes**:
- The forward rate (Rf) is initially high because there are plenty of reactants (A and B) available.
- As the reaction continues, the concentration of A and B decreases, leading to a decrease in the forward rate (Rf).
- Conversely, the backward rate (Rb) starts at zero (since C and D are initially absent) and increases as C and D are formed.

5. **Equilibrium State**:
- Eventually, a point is reached where the forward rate (Rf) equals the backward rate (Rb). This is the state of chemical equilibrium.
- At equilibrium, the concentrations of A, B, C, and D remain constant over time, even though the forward and backward reactions continue to occur.

6. **Graphical Representation**:
- The rate of reaction can be plotted on a graph with time on the x-axis and reaction rate on the y-axis.
- The curve for the forward reaction (Rf) will start high and decrease over time, while the curve for the backward reaction (Rb) will start at zero and increase.
- The point where the two curves intersect represents the equilibrium point.