A Nitrogen oxide, NO, reacts with bromine to give nitrosyl bromide, NOBr 2NO (g)

Question

A Nitrogen oxide, NO, reacts with bromine to give nitrosyl bromide, NOBr 2NO (g) + Br_2(g) 2NOBr (g) A one liter flask which contains NO and Br_2 is allowed to reach equilibrium at a certain temperature. At equilibrium, the total pressure in the flask is 2.62 atm. The equilibrium partial pressure of NO and Br_2 are 0.860 atm and 0.573 atm respectively. Calculate K fro the reaction at the temperature of the experiment. Consider the equation above as written. Circle the answer to show in which direction will the reaction proceed if more NO is added. the volume of the flask is increased to 2.0 L more NOBr is added.

Explanation / Answer

2 NO (g) + Br2 (g) = 2 NOBr (g)

At equilibrium, PNO = 0.860 atm
PBr2 = 0.573 atm

Total P = 2.62 atm

then, PNOBr = 2.62 - 0.860 - 0.573 = 1.187 atm

Equilibrium constant expression interms of pressure can be written as,

Kp = PNOBr2 / (PNO2 * PBr2)

Kp = (1.187)2 / [(0.860)2 * (0.573)]

Kp = 3.32

(2)

More NO is added => shifts towards right side

Volume is increased to 2.0 L=> shifts towards left ( more umber of gas substances)

More NOBr is added => shifts towards left

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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