O www.we ortes here, select then and drag to the Favorites Bar folder. Or import

Question

O www.we ortes here, select then and drag to the Favorites Bar folder. Or import from another browser. Import favorites GilChem5 14P 083 A flask containing pure NO2 was heated to 1000 K, a temperature at which the value of Kp for the decomposition of NO2 is 158. 2 NO2(g) 2 NO(g) + 02(g) The partial pressure of 02 at equilibrium is 0.245 atm. (a) Calculate the partial pressures of NO and NO2. PNo 0.49 atm 49 Xatm (b) Calculate the total pressure in the flask at equilibrium. atm 5 14 P 088 On a very smoggy day, the equilibrium concentration of NO2 in the air over an urban area reaches 2.2 x 10 M. If the temperature

Explanation / Answer

Partial pressure of O2, p(O2) = 0.245 atm

2 NO2 ó 2 NO + O2

(Po – 2 x) ó 2 x + x

a)

p(NO) = 2 * p(O2)

= 2 * 0.245 atm = 0.49 atm

At equilibrium,

Kp = p(O2) * p(NO)2 / p(NO2)2 = 158

0.245 * 0.492 / p(NO2)2 = 158

p(NO2)2 = 0.00037 atm

p(NO2) = 0.019 atm

b)

Total pressure at equilibrium = p(O2) + p(NO) + p(NO2)

= 0.245 + 0.49 + 0.019 atm

= 0.754 atm

Related Questions

Navigate

• Browse (All)
• Browse O
• Subjects

---

---

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