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a)  For the reaction : $$2A\left( g \right) +B\left( g \right) \longrightarrow 2D\left( g \right) $$,  $$\Delta U=-10.5\quad kJ$$ and $$\Delta S=-44.1\quad { kJ }^{ -1 }$$. Calculate $$\Delta G$$ for the reaction, and predict whether the reaction may occur spontaneously.
b)  Predict whether the reaction is spontaneous or not at high temperature.


Solution

Given that $$2A+B\longrightarrow 2D_{(g)}$$       $$\Delta U= -10.5 kJ$$
$$\Delta ng= np-nr$$
         $$=2-(2+1)=-1$$
$$\Delta H= \Delta U^o+\Delta ngRT$$
         $$=-10.5+(-1)0.008314 \times 298=-12.947 kJ$$
$$\Delta G= \Delta H-J \Delta S$$
        $$=-12.947-298\times (-44\times 10^{-3})=0.165 kJ$$

$$\Delta G$$ is positive, then the reaction won't occur spontaneously.

Chemistry

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