For an ideal gas, under isobaric condition, a graph between log V vs log T :

Options

A. is linear with unit slope
B. represents Boyle’s Law
C. represents Charle’s Law
D. represents Gay-Lussac’s Law

Explanation

To solve the question regarding the graph between log V vs log T for an ideal gas under isobaric conditions, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Conditions**: We are dealing with an ideal gas under isobaric conditions, which means the pressure (P) is constant.

2. **Apply Charles's Law**: According to Charles's Law, for an ideal gas at constant pressure, the volume (V) of the gas is directly proportional to its absolute temperature (T). This can be expressed mathematically as:
\[ V \propto T \quad \text{or} \quad V = kT \]
where \(k\) is a constant.

3. **Take the Logarithm**: To analyze the relationship in logarithmic terms, we take the logarithm of both sides:
\[ \log V = \log(kT) \]

4. **Use Logarithmic Properties**: Using the property of logarithms that states \(\log(ab) = \log a + \log b\), we can rewrite the equation:
\[ \log V = \log k + \log T \]

5. **Identify the Graph Components**: In this equation, \(\log V\) is on the y-axis and \(\log T\) is on the x-axis. This can be rearranged to the form of a straight line:
\[ \log V = \log k + 1 \cdot \log T \]
Here, the slope (m) is 1 and the y-intercept (c) is \(\log k\).

6. **Conclusion about the Graph**: Since the relationship is linear, we conclude that the graph of \(\log V\) versus \(\log T\) will be a straight line with a slope of 1.

### Final Answer:
The graph between log V vs log T for an ideal gas under isobaric conditions is a linear graph with a unit slope.