What is the magnitude of ΔH° for the decomposition of 2 moles of nitroglycerin at 25°C?

What is the magnitude of ΔH° for the decomposition of 2 moles of nitroglycerin at 25°C?

• A. 500 kJ
• B. 1000 kJ
• C. 2000 kJ
• D. 3000 kJ

Answer: (D)

To determine the magnitude of ΔH° for the decomposition of 2 moles of nitroglycerin at 25°C, it's essential to reference the known thermodynamic data for nitroglycerin, which is typically provided in tables related to standard enthalpies of formation. The decomposition reaction of nitroglycerin can be represented as: \[ 4 \text{C}_3\text{H}_5\text{N}_3\text{O}_9 \rightarrow 6 \text{C} + 10 \text{H}_2\text{O} + 6 \text{N}_2 + 5 \text{O}_2 \] For nitroglycerin, the ΔH° for its decomposition is a large positive value because it is an exothermic reaction, meaning it releases a significant amount of energy upon decomposition. From thermodynamic reference tables, the ΔH° for the decomposition of 1 mole of nitroglycerin is approximately 1471 kJ/mol. Therefore, for 2 moles of nitroglycerin, the total energy released or ΔH° becomes: \[ 2 \text{ moles} \times 1471 \text{ k

To determine the magnitude of ΔH° for the decomposition of 2 moles of nitroglycerin at 25°C, it's essential to reference the known thermodynamic data for nitroglycerin, which is typically provided in tables related to standard enthalpies of formation.

The decomposition reaction of nitroglycerin can be represented as:

[ 4 \text{C}_3\text{H}_5\text{N}_3\text{O}_9 \rightarrow 6 \text{C} + 10 \text{H}_2\text{O} + 6 \text{N}_2 + 5 \text{O}_2 ]

For nitroglycerin, the ΔH° for its decomposition is a large positive value because it is an exothermic reaction, meaning it releases a significant amount of energy upon decomposition.

From thermodynamic reference tables, the ΔH° for the decomposition of 1 mole of nitroglycerin is approximately 1471 kJ/mol. Therefore, for 2 moles of nitroglycerin, the total energy released or ΔH° becomes:

[ 2 \text{ moles} \times 1471 \text{ k