# Problem: Consider the system: 2 N2O5(g) ⇌ 2N2O4(g) + O2(g) at equilibrium at 25°C. If this is an exothermic reaction and the temperature was raised, would the equilibrium be shifted to produce more N2O5 or more N2O4? it is impossible to tell there would be no change more  N2O5 more N2O4

🤓 Based on our data, we think this question is relevant for Professor Seivert's class at UGA.

###### Problem Details

Consider the system:

2 N2O5(g) ⇌ 2N2O4(g) + O2(g)

at equilibrium at 25°C. If this is an exothermic reaction and the temperature was raised, would the equilibrium be shifted to produce more N2O5 or more N2O4?

1. it is impossible to tell
2. there would be no change
3. more  N2O5
4. more N2O4

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Le Chatelier's Principle concept. You can view video lessons to learn Le Chatelier's Principle . Or if you need more Le Chatelier's Principle practice, you can also practice Le Chatelier's Principle practice problems.

What is the difficulty of this problem?

Our tutors rated the difficulty ofConsider the system: 2 N2O5(g) ⇌ 2N2O4(g) + O2(g) at equil...as medium difficulty.

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What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Seivert's class at UGA.