For the reaction

2A(g) + B(g)→ 2D(g)

$$\Delta U^{\Theta } = -10.5 kJ \;and \;\Delta S^{\Theta } = -44.1JK^{-1}$$

Calculate $$\Delta G^{\Theta }$$ for the reaction, and predict whether the reaction may occur spontaneously.

Asked by Abhisek | 1 year ago |  166

Solution :-

2A(g) + B(g) → 2D(g)

$$\Delta n_{g} = 2 – 3$$

= -1 mole

Putting value of $$\Delta U^{\Theta }$$ in expression of $$\Delta H$$:

$$\Delta H^{\Theta } = \Delta U^{\Theta } + \Delta n_{g}RT$$

= (-10.5KJ) – (-1)

$$( 8.314\times 10^{-3}kJK^{-1}mol^{-1}$$(298K)

= -10.5kJ -2.48kJ

$$\Delta H^{\Theta }$$ = -12.98kJ

Putting value of $$\Delta S^{\Theta }$$ and$$\Delta H^{\Theta }$$ in expression of$$\Delta G^{\Theta }$$:

$$\Delta G^{\Theta } = \Delta H^{\Theta } – T\Delta S^{\Theta }$$

= -12.98kJ –(298K)$$(-44.1JK^{-1})$$

= -12.98kJ +13.14kJ

$$\Delta G^{\Theta }$$ = 0.16kJ

As, $$\Delta G^{\Theta }$$ is positive, the reaction won’t occur spontaneously.

Answered by Pragya Singh | 1 year ago

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