QuestionMay 14, 2025

9. (6 points)Using two or more of the following reactions. N2(g)+3/2O2(g)arrow N2O3(g)Delta H=+83.7kJ N2(g)+O2(g)arrow 2NO(g)Delta H=+180.4kJ 1/2N2(g)+O2(g)arrow NO2(g)Delta H=+33.2kJ Determine the Delta H^circ of the following reaction: NO(g)+NO2(g)arrow N2O3(g)Delta H=?

9. (6 points)Using two or more of the following reactions. N2(g)+3/2O2(g)arrow N2O3(g)Delta H=+83.7kJ N2(g)+O2(g)arrow 2NO(g)Delta H=+180.4kJ 1/2N2(g)+O2(g)arrow NO2(g)Delta H=+33.2kJ Determine the Delta H^circ of the following reaction: NO(g)+NO2(g)arrow N2O3(g)Delta H=?
9. (6 points)Using two or more of the following reactions. N2(g)+3/2O2(g)arrow N2O3(g)Delta H=+83.7kJ N2(g)+O2(g)arrow 2NO(g)Delta H=+180.4kJ 1/2N2(g)+O2(g)arrow NO2(g)Delta H=+33.2kJ Determine the Delta H^circ of the following reaction: NO(g)+NO2(g)arrow N2O3(g)Delta H=?

Solution
4.7(202 votes)

Answer

\Delta H^{\circ } = -63.5 \text{ kJ} Explanation 1. Write Target Reaction The target reaction is NO(g) + NO2(g) \rightarrow N2O3(g). 2. Use Given Reactions We need to combine the given reactions to form the target reaction. 3. Reverse and Adjust Reactions Reverse the second reaction: 2NO(g) \rightarrow N2(g) + O2(g), \Delta H = -180.4 \text{ kJ}. Use the third reaction as is: 1/2N2(g) + O2(g) \rightarrow NO2(g), \Delta H = +33.2 \text{ kJ}. 4. Combine Reactions Add the reversed second reaction and the third reaction: - 2NO(g) \rightarrow N2(g) + O2(g), \Delta H = -180.4 \text{ kJ} - 1/2N2(g) + O2(g) \rightarrow NO2(g), \Delta H = +33.2 \text{ kJ} This results in: - 2NO(g) + 1/2N2(g) + O2(g) \rightarrow N2(g) + O2(g) + NO2(g) 5. Simplify and Match Target Reaction Simplify to match the target reaction: - NO(g) + NO2(g) \rightarrow N2O3(g) 6. Calculate \Delta H^{\circ } Combine the enthalpy changes: - \Delta H = (-180.4 \text{ kJ}) + (33.2 \text{ kJ}) + (83.7 \text{ kJ})

Explanation

1. Write Target Reaction<br /> The target reaction is $NO(g) + NO2(g) \rightarrow N2O3(g)$.<br /><br />2. Use Given Reactions<br /> We need to combine the given reactions to form the target reaction. <br /><br />3. Reverse and Adjust Reactions<br /> Reverse the second reaction: $2NO(g) \rightarrow N2(g) + O2(g)$, $\Delta H = -180.4 \text{ kJ}$.<br /> Use the third reaction as is: $1/2N2(g) + O2(g) \rightarrow NO2(g)$, $\Delta H = +33.2 \text{ kJ}$.<br /><br />4. Combine Reactions<br /> Add the reversed second reaction and the third reaction:<br />- $2NO(g) \rightarrow N2(g) + O2(g)$, $\Delta H = -180.4 \text{ kJ}$<br />- $1/2N2(g) + O2(g) \rightarrow NO2(g)$, $\Delta H = +33.2 \text{ kJ}$<br /><br /> This results in:<br />- $2NO(g) + 1/2N2(g) + O2(g) \rightarrow N2(g) + O2(g) + NO2(g)$<br /><br />5. Simplify and Match Target Reaction<br /> Simplify to match the target reaction:<br />- $NO(g) + NO2(g) \rightarrow N2O3(g)$<br /><br />6. Calculate $\Delta H^{\circ }$<br /> Combine the enthalpy changes:<br />- $\Delta H = (-180.4 \text{ kJ}) + (33.2 \text{ kJ}) + (83.7 \text{ kJ})$
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