For the reaction 2NOBr(g) doubleheadarrow 2NO (g) + Br_2(g), Delta H degree _rxn

Question

For the reaction 2NOBr(g) doubleheadarrow 2NO (g) + Br_2(g), Delta H degree _rxn = +30 kJ/mol. At equilibrium, which one of the changes below would cause the equilibrium to shift to the left? A) Increase the container volume. B) Remove some NO. C) Remove some Br_2. D) Add more NOBr. E) Decrease the temperature. For the reaction at equilibrium: 2SO_2(g) + O_2(g) doubleheadarrow 2SO_3 (g), Delta H degree _rxn = -198 kJ/mol. If the volume of the system is compressed at constant temperature, what change will occur in the position of the equilibrium? A) A shift to produce more SO_2 B) A shift to produce more O_2 C) No change D) A shift to produce more SO_3

Explanation / Answer

Q9.

this is endothermic, meaning it requires heat to produce products

so..

a increasing V, will favour the most moles of gas formation, which is for product, since it has 2+1 = 3 moles of gas

shift goes to right side

b)

removing products will make the reaction shift toward more production of NO and Br2

c)

removing products will make the reaction shift toward more production of NO and Br2

d)

adding NOBr, a reactants, will make the reaction shift toward more production of NO and Br2, since there is plenty of reagents

e)

If we decrease T, we will favour less production, since this is endothermic, so more reactants will be produced

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

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