Given the reactions:
1) ½N₂(g) + ½O₂(g) → NO(g); Δ_r H° = 90 kJ mol⁻¹
2) NO(g) + ½O₂(g) → NO₂(g); Δ_

Q: What is the correct answer for CBSE11?

The correct answer is B. This is Exercise 5.21. For NO(g) to be stable, its formation from elements should be exothermic (negative Δ_f H°) or it should not readily decompose or react further. Reaction 1 shows that the formation of NO(g) from its elements is endothermic (Δ_r H° = +90 kJ mol⁻¹). This suggests it is less stable. Reaction 2 shows that NO(g) readily reacts with O₂(g) to form NO₂(g) with a negative Δ_r H° (-74

Q: Given the reactions: 1) ½N₂(g) + ½O₂(g) → NO(g); Δ_r H° = 90 kJ mol⁻¹ 2) NO(g) + ½O₂(g) → NO₂(g); Δ_r H° = -74 kJ mol⁻¹ Comment on the thermodynamic stability of NO(g).

The correct answer is B. This is Exercise 5.21. For NO(g) to be stable, its formation from elements should be exothermic (negative Δ_f H°) or it should not readily decompose or react further. Reaction 1 shows that the formation of NO(g) from its elements is endothermic (Δ_r H° = +90 kJ mol⁻¹). This suggests it is less stable. Reaction 2 shows that NO(g) readily reacts with O₂(g) to form NO₂(g) with a negative Δ_r H° (-74

Q: What are the options for this CBSE11 question?

A. NO(g) is thermodynamically stable because its formation is endothermic. · B. NO(g) is thermodynamically unstable because its formation from elements is endothermic and it readily reacts to form NO₂. · C. NO(g) is thermodynamically stable because its decomposition is exothermic. · D. NO(g) is thermodynamically unstable because its formation from elements is exothermic.

Question

Given the reactions:
1) ½N₂(g) + ½O₂(g) → NO(g); Δ_r H° = 90 kJ mol⁻¹
2) NO(g) + ½O₂(g) → NO₂(g); Δ_r H° = -74 kJ mol⁻¹
Comment on the thermodynamic stability of NO(g).

FirstInTest · Accepted Answer

This is Exercise 5.21. For NO(g) to be stable, its formation from elements should be exothermic (negative Δ_f H°) or it should not readily decompose or react further. Reaction 1 shows that the formation of NO(g) from its elements is endothermic (Δ_r H° = +90 kJ mol⁻¹). This suggests it is less stable. Reaction 2 shows that NO(g) readily reacts with O₂(g) to form NO₂(g) with a negative Δ_r H° (-74 kJ mol⁻¹), indicating a spontaneous and favorable reaction. Both points suggest NO(g) is thermodynamically unstable.

Answer

NO(g) is thermodynamically stable because its formation is endothermic.

Answer

NO(g) is thermodynamically unstable because its formation from elements is endothermic and it readily reacts to form NO₂.

Answer

NO(g) is thermodynamically stable because its decomposition is exothermic.

Answer

NO(g) is thermodynamically unstable because its formation from elements is exothermic.

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