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(C) According to the Clausius-Clapeyron equation,the relationship between vapour pressure $(p)$ and absolute temperature $(T)$ is given by:$\log p = -

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(C) According to the Clausius-Clapeyron equation,the relationship between vapour pressure $(p)$ and absolute temperature $(T)$ is given by:$\log p = -\frac{\Delta H_{vap}}{2.303 R} \cdot \frac{1}{T} + C$Here,$\Delta H_{vap}$ is the enthalpy of vaporization,$R$ is the gas constant,and $C$ is an integration constant.This equation is in the form of a straight line $y = mx + c$,where $y = \log p$,$x = \frac{1}{T}$,and the slope $m = -\frac{\Delta H_{vap}}{2.303 R}$.Since the slope is negative,the graph of $\log p$ versus $\frac{1}{T}$ is a straight line with a negative slope.

Which one of the following represents the graph between $\log p$ (on $Y$-axis) and $\frac{1}{T}$ (on $X$-axis)?
($p=$ vapour pressure of a liquid,$T=$ absolute temperature)

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Which one of the following represents the graph between $\log p$ (on $Y$-axis) and $\frac{1}{T}$ (on $X$-axis)?($p=$ vapour pressure of a liquid,$T=$ absolute temperature)