Nitrogen and oxygen react to form nitrogen monoxide, like this: N 2(g) +02(g) 2N

Question

Nitrogen and oxygen react to form nitrogen monoxide, like this: N 2(g) +02(g) 2NO(g) The reaction is endothermic. Suppose a mixture of N2, O2 and NO has come to equilibrium in a closed reaction vessel. Predict what change , if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium to the right to the left (none) to the right The temperature is lowered The pressure of N2 will ? The pressure of NO will A catalyst is added to the The pressure of N2 will reaction vessel. to the left The pressure of NO will (none)

Explanation / Answer

1)

Forward reaction is endothermic in nature

we are decreasing temperature or removing heat here

so, according to Le Chatelier's principle,

equilibrium will move in direction which release heat

hence, backward reaction will be favoured

Equilibrium moves to left

The pressure of N2 increases

The pressure of NO decreases

shift in equilibrium: to the left

2)

Catalyst doesn't affect equilibrium

No effect on equilibrium

The pressure of N2 doesn’t change

The pressure of NO doesn’t change

shift in equilibrium: none

Feel free to comment below if you have any doubts or if this answer do not work

Related Questions

Navigate

• Browse (All)
• Browse N
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.