11) For which of the following reaction or reactions would you expect the extent of the forward reaction to increase with increasing temperatures? (5P) (a) $PCl_5(g) ightleftharpoons PCl_3(g) + Cl_2(g)$ $Delta H^o = +92.5 ext{ kJ}$ (b) $SO_3(g) ightleftharpoons SO_2(g) + frac{1}{2}O_2(g)$ $Delta H^o = +98.9 ext{ kJ}$ (c) $N_2H_4(g) ightleftharpoons N_2(g) + 2H_2(g)$ $Delta H^o = -95.4 ext{ kJ}$ (d) $COCl_2(g) ightleftharpoons CO(g) + Cl_2(g)$ $Delta H^o = +108.3 ext{ kJ}$ a) A b) B c) C d) D
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We need to identify which reactions will have an increased extent of the forward reaction with increasing temperatures. This involves understanding the relationship between temperature and the direction of reaction shifts as described by Le Chatelier's Principle. Show more…
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For which of the following reactions would you expect the extent of the forward reaction to increase with increasing temperatures? Explain. (a) $\quad \mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{N}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=-90.2 \mathrm{kJ}$ (b) $\quad \mathrm{SO}_{3}(\mathrm{g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=+98.9 \mathrm{kJ}$ (c) $\mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{g}) \rightleftharpoons \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=-95.4 \mathrm{kJ}$ (d) $\mathrm{COCl}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g}) \quad \Delta H^{\circ}=+108.3 \mathrm{kJ}$
For which of the following reactions would you expect the extent of the forward reaction to increase with increasing temperatures? Explain. (a) $\quad \mathrm{NO}(\mathrm{g}) \rightleftharpoons \frac{1}{2} \mathrm{N}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \quad \Delta_{\mathrm{r}} H^{\circ}=-90.2 \mathrm{kJ} \mathrm{mol}^{-1}$ (b) $\quad \mathrm{SO}_{3}(\mathrm{g}) \rightleftharpoons \mathrm{SO}_{2}(\mathrm{g})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{g}) \quad \Delta_{\mathrm{r}} H^{\circ}=+98.9 \mathrm{kJ} \mathrm{mol}^{-1}$ (c) $\quad \mathrm{N}_{2} \mathrm{H}_{4}(\mathrm{g}) \rightleftharpoons \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2}(\mathrm{g}) \quad \Delta_{\mathrm{r}} H^{\circ}=-95.4 \mathrm{kJ} \mathrm{mol}^{-1}$ (d) $\operatorname{COCl}_{2}(\mathrm{g}) \rightleftharpoons \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{g}) \quad \Delta_{\mathrm{r}} H^{\circ}=+108.3 \mathrm{kJ} \mathrm{mol}^{-1}$
Consider the following reactions. In which cases is product formation favoured by decreased temperature? (1) $\mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{NO}(g) ; \quad \Delta H^{\circ}=181 \mathrm{~kJ}$ (2) $2 \mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) ; \quad \Delta H^{\circ}=566 \mathrm{~kJ}$ (3) $\mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g)$ $\Delta H^{\circ}=-9.4 \mathrm{~kJ}$ (4) $\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g) ; \quad \Delta H^{\circ}=-541 \mathrm{~kJ}$ (a) 1,2 (b) 2 only (c) $1,2,3$ (d) 3,4
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