A gas obeying the Clausius equation of state is isothermally compressed from $5\:Mpa$ to $15\:MPa$ in a closed system at $400\:K$. The Clausius equation of state is $P=\frac{RT}{v-b\left ( T \right )}$ where $P$ is the pressure, $T$ is the temperature, $v$ is the molar volume and $R$ is the universal gas constant. The parameter $b$ in the above equation varies with temperature as $b(T)=b_{0}+b_{1}T$ with $b_{0}=4\times 10^{-5}$ $m^{3} mol^{-1} $and $b_{1}=1.35\times 10^{-7}$ $m^{3}$ mol$^{-1}\:K^{-1}$. The effet of pressure on the molar enthapy $(h)$ at a constant temperature is given by $\left ( \frac{\partial h}{\partial P} \right )_{T}=v-T\left ( \frac{\partial v}{\partial T} \right )_{P}$. Let $h_{i}$ and $h_{f}$ denote the initial and final molar enthalpies, respectively. The change in the molar enthalpy $h_{f}-h_{i}$ (in $J$ mol$^{-1}$, rounded off to the first decimal place) for this process is ______________