Question

Consider the decomposition of gaseous $\mathrm{N}_{2} \mathrm{O}_{4}$: $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \quad \Delta H^{\circ}=+55.3 \mathrm{kJ} ; \Delta S^{\circ}=+175.7 \mathrm{J} / \mathrm{K}$$ (a) Is this reaction spontaneous under standard-state conditions at $25^{\circ} \mathrm{C} ?$ (b) Estimate the temperature at which the reaction becomes spontaneous.

          Consider the decomposition of gaseous $\mathrm{N}_{2} \mathrm{O}_{4}$:
$$\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \quad \Delta H^{\circ}=+55.3 \mathrm{kJ} ; \Delta S^{\circ}=+175.7 \mathrm{J} / \mathrm{K}$$
(a) Is this reaction spontaneous under standard-state conditions at $25^{\circ} \mathrm{C} ?$
(b) Estimate the temperature at which the reaction becomes spontaneous.

Added by Robin A.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Sri K

03/31/2023

Step 1

(a) At $25^{\circ} \mathrm{C}$, the temperature is $298 \mathrm{K}$. Plugging in the given values, we get:$$\Delta G^{\circ} = (55.3 \times 10^3 \mathrm{J}) - (298 \mathrm{K})(175.7 \mathrm{J}/\mathrm{K})$$Calculating the result, we find:$$\Delta G^{\circ} = Show more…

Show all steps

Thanks for your feedback!

Consider the decomposition of gaseous $\mathrm{N}_{2} \mathrm{O}_{4}$: $$\mathrm{N}_{2} \mathrm{O}_{4}(g) \longrightarrow 2 \mathrm{NO}_{2}(g) \quad \Delta H^{\circ}=+55.3 \mathrm{kJ} ; \Delta S^{\circ}=+175.7 \mathrm{J} / \mathrm{K}$$ (a) Is this reaction spontaneous under standard-state conditions at $25^{\circ} \mathrm{C} ?$ (b) Estimate the temperature at which the reaction becomes spontaneous.