A schematic plot of $\ln K_c$ versus inverse of temperature for reaction is shown below
Which of the following statement(s) is/are correct regarding the reaction?

$xA\rightleftarrows yB K_C=\frac{{\left[B\right]}^y}{{\left[A\right]}^x}$

 

 

 

 

 

 

$$\begin{gathered} \ln K_c=\frac{-\Delta H^0}{RT}+\frac{T\Delta S^0}{RT} \\ \ln K_c=\frac{-\Delta H^0}{R}\left(\frac{1}{T}\right)+\frac{\Delta S^0}{R} \\ y = m x + c \end{gathered}$$

slope of curve is negative it means $\Delta H^0$ is positive and value of $K_c$ is less than unity hence, reaction is non-spontaneous at standard condition