NEET2026PhysicsChapterActual
The given figure shows the volume ( V ) versus absolute temperature ( T ) graphs for equal masses of three different ideal gases A, B, and C, measured at the same constant pressure. If M_A , M_B , and M_C are their respective molar masses, which of the following relations is correct?
Options
- AM_A > M_B > M_C
- BM_A < M_B < M_C
- CM_A = M_B = M_C
- DM_B > M_C > M_A
Correct answer
B. M_A < M_B < M_C
Step-by-step solution
According to the ideal gas equation, PV = nRT . Substituting the number of moles n = m M , where m is the mass and M is the molar mass, we get: PV = m M RT Rearranging this equation to represent the volume V as a function of absolute temperature T , we have: V = ( mR PM )T This represents a straight line passing through the origin with a slope given by: Slope = mR PM Since the mass m and pressure P are constant for all three gases, the slope is inversely proportional to the molar mass M : Slope 1 M From the given V