Which of the following graph ploltted between `P` and `V` is
INCORRECT ?

Options

A.
B.
C.
D. None of these

Explanation

To determine which graph plotted between pressure (P) and volume (V) is incorrect, we need to analyze the graphs based on the gas laws.

### Step-by-Step Solution:

1. **Understanding Boyle's Law**:
- Boyle's Law states that for a given mass of gas at constant temperature, the pressure (P) is inversely proportional to the volume (V). This can be mathematically expressed as:
\[ PV = k \quad (k \text{ is a constant}) \]
- Therefore, if we plot P against V, the graph should be a hyperbola that approaches both axes but never touches them.

2. **Analyzing the First Graph**:
- The first graph shows a hyperbolic relationship between P and V.
- Since it follows Boyle's Law (P inversely proportional to V at constant temperature), this graph is **correct**.

3. **Understanding Charles's Law**:
- Charles's Law states that at constant pressure, the volume (V) of a gas is directly proportional to its temperature (T). This can be expressed as:
\[ \frac{V}{T} = k \quad (k \text{ is a constant}) \]
- If we plot V against T at constant pressure, the graph should be a straight line.

4. **Analyzing the Second Graph**:
- The second graph depicts a scenario where pressure is held constant while volume changes with temperature.
- If the order of temperatures is T1, T2, T3, and the volume is increasing, this suggests that the temperature is also increasing. However, if the graph suggests otherwise (like T3 being the lowest temperature), this indicates a contradiction with Charles's Law.
- Therefore, this graph is **incorrect**.

5. **Analyzing the Third Graph**:
- The third graph again shows a hyperbolic relationship similar to the first graph.
- Since it also follows Boyle's Law, this graph is **correct**.

### Conclusion:
The incorrect graph plotted between P and V is the **second graph**.