For the reaction 2NO(g)+ O 2 (g)$\rarr$ 2NO 2 (g), $\Delta$H° = -113.1 kJ/mol and $\Delta$S° = -145.3 J/K mol.Which of these statements is true?

The reaction is exothermic ($\Delta$H° < 0) and has a negative entropy change ($\Delta$S° < 0). It is spontaneous at low temperatures where the enthalpy term dominates.

For the reaction 2NO(g)+ O 2 (g)$\rarr$ 2NO 2 (g), $\Delta$H° = -113.1 kJ/mol and $\Delta$S° = -145.3 J/K mol.Which of these statements is true?

The reaction is exothermic ($\Delta$H° < 0) and has a negative entropy change ($\Delta$S° < 0). It is spontaneous at low temperatures where the enthalpy term dominates.

Solved

For the Reaction 2NO(g)+ O₂(g) $\rarr$ 2NO₂(g) $\Delta$ H° = -1131 KJ/mol And 2NO(g)

Question 33

Multiple Choice

For the reaction 2NO(g) + O₂(g) $\rarr$ 2NO₂(g) , $\Delta$ H° = -113.1 kJ/mol and $\Delta$ S° = -145.3 J/K mol.Which of these statements is true?

A) The reaction is spontaneous at all temperatures.
B) The reaction is only spontaneous at low temperatures.
C) The reaction is only spontaneous at high temperatures.
D) The reaction is at equilibrium at 25°C under standard conditions.
E) $\Delta$ G° becomes more favorable as temperature increases.

Correct Answer: