Question:
At constant temperature, the product \(PV\) is plotted against pressure \(P\) for an ideal gas. The graph obtained is
At constant temperature, the product \(PV\) is plotted against pressure \(P\) for an ideal gas. The graph obtained is
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For an ideal gas at constant temperature, \(PV\) remains constant, so the \(PV\) versus \(P\) graph is horizontal.
Updated On: May 7, 2026
- Straight line parallel to \(P\)-axis
- Straight line with positive slope
- Straight line through origin
- Parabola
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The Correct Option is A
Solution and Explanation
Concept:
For an ideal gas:
\[
PV=nRT
\]
Step 1: At constant temperature: \[ T=\text{constant} \] Also, for a fixed amount of gas: \[ n=\text{constant} \] Therefore: \[ PV=nRT=\text{constant} \]
Step 2: This means the value of \(PV\) does not change with pressure \(P\).
Step 3: If \(PV\) is plotted on the vertical axis and \(P\) on the horizontal axis, then \(PV\) remains constant for all values of \(P\). So the graph is a horizontal straight line.
Step 4: A horizontal line is parallel to the \(P\)-axis. Therefore: \[ \boxed{\text{Straight line parallel to }P\text{-axis}} \]
Step 1: At constant temperature: \[ T=\text{constant} \] Also, for a fixed amount of gas: \[ n=\text{constant} \] Therefore: \[ PV=nRT=\text{constant} \]
Step 2: This means the value of \(PV\) does not change with pressure \(P\).
Step 3: If \(PV\) is plotted on the vertical axis and \(P\) on the horizontal axis, then \(PV\) remains constant for all values of \(P\). So the graph is a horizontal straight line.
Step 4: A horizontal line is parallel to the \(P\)-axis. Therefore: \[ \boxed{\text{Straight line parallel to }P\text{-axis}} \]
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