Solution Found!
The equilibrium constant (KP) for the reaction is 4.0 ×
Chapter 20, Problem 68P(choose chapter or problem)
The equilibrium constant \(\left(K_{P}\right)\) for the reaction
\(\mathrm{N}_2(g)+\mathrm{O}_2(g)\ \rightleftharpoons\ 2\mathrm{NO}(g)\)
is \(4.0 \times 10^{-31}\) at \(25^{\circ} \mathrm{C}\) and \(2.6 \times 10^{-6}\) at \(1100^{\circ} \mathrm{C}\), the temperature of a running car's engine. Is this an endothermic or exothermic reaction?
Questions & Answers
QUESTION:
The equilibrium constant \(\left(K_{P}\right)\) for the reaction
\(\mathrm{N}_2(g)+\mathrm{O}_2(g)\ \rightleftharpoons\ 2\mathrm{NO}(g)\)
is \(4.0 \times 10^{-31}\) at \(25^{\circ} \mathrm{C}\) and \(2.6 \times 10^{-6}\) at \(1100^{\circ} \mathrm{C}\), the temperature of a running car's engine. Is this an endothermic or exothermic reaction?
ANSWER:Step 1 of 2
We need to explain whether the given reaction is an exothermic or endothermic reaction.
Given the reaction
And the equilibrium constants
