Question

Which one of the following graphs is not correct for an ideal gas?

• A. $\left(\mathrm{i}\right)$
• B. $\left(\mathrm{iv}\right)$
• C. $\left(\mathrm{iii}\right)$
• D. $\left(\mathrm{ii}\right)$

Answer 1

The correct option is D

$\left(\mathrm{ii}\right)$

The correct statement is (d):

The explanation for the correct options:

(d)

• Explanation: In the case of an ideal gas. The plot of d versus 1/T is not a straight line. A curved line is not the same as a straight line. When a point does not go in one direction, it forms a curve.
• According to Robert Boyle's law, a sample at equilibrium has pressure and volume values that are constant.
  
• $\mathrm{PM}=\mathrm{dRT}$
• $\mathrm{d}=\left[\frac{\mathrm{PM}}{\mathrm{R}}\right]\frac{1}{\mathrm{T}}$
• Diagram:

The explanation for the incorrect options:

(a)

• Explanation: In order to have flawless gas. The graph between d and T is hyperbolic. A hyperbola is utilized instead of a circle. The points, like the radius of a circle with a unit radius, make up the right side of the unit hyperbola.
• $\mathrm{d}=\left[\begin{array}{cc}\mathrm{P}\times & \mathrm{M}\end{array}\right]/\mathrm{RT}$
• Diagram:

(b)

• Explanation: For an ideal gas. the graph between d Vs P is a straight line. A straight line is simply one that is devoid of bends. A straight line is defined as a line that extends indefinitely on both sides and has no bends.
• $\mathrm{d}=\left[\begin{array}{cc}\mathrm{P}\times & \mathrm{M}\end{array}\right]/\mathrm{RT}$
• Diagram:

(c)

• Explanation: For a perfect gas. The graph of d as a function of 1/T is a straight line.
• There are no curves in a straight line. A straight line is one that has no bends and stretches to infinity on both sides.
• $\mathrm{d}=\left[\begin{array}{cc}\mathrm{P}\times & \mathrm{M}\end{array}\right]/\mathrm{RT}$
• Diagram:

The correct statement is (d): The plot of d versus T is not a straight line.