a) N2(g) + O2(g) 2NO (g) ∆H298 = + 180 kJ mol-1 From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by: Increasing the concentration of NO Increasing the pressure Increasing the temperature Increasing the concentration of N2 Adding a catalyst
a) N2(g) + O2(g) 2NO (g) ∆H298 = + 180 kJ mol-1 From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by: Increasing the concentration of NO Increasing the pressure Increasing the temperature Increasing the concentration of N2 Adding a catalyst
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter12: Chemical Equilibrium
Section: Chapter Questions
Problem 12.45PAE: The following equilibrium is established in a closed container: C(s)+O2(g)CO2(g)H=393kJmol1 How does...
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(a) N2(g) + O2(g) 2NO (g) ∆H298 = + 180 kJ mol-1
From the equilibrium shown above, use Le Chatelier’s Principle to decide what happens to the equilibrium position by:
- Increasing the concentration of NO
- Increasing the pressure
- Increasing the temperature
- Increasing the concentration of N2
- Adding a catalyst
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