32. Consider the following reaction: 2NO2(g) 2N0(g) + O2(g) Starting with pure N

Question

32. Consider the following reaction: 2NO2(g) 2N0(g) + O2(g) Starting with pure NO2(g) at a pressure of 0.500 atm, at equilibrium the taisl per was 0.732 atm. Calculate the equilibrium partial pressure of NOB) A) 0.0360 atm B) 0.232 atm C) 0.464 atm D) 0.400 atm E) 0.493 atm 33. Consider the following reaction at a certain temperature: PCI5(g) t PC13(g) + Cl (g) Ke-00736 At equilibrium, [PCIs]-0.110 M and [PCI3]-[C2]-0.0900 M. If suddenly 0.100 M PCIs(g), PCl3(8) and Cl2(8) were added, which of the following is true? A) More products will be formed. B) [C2l-0.190 M at equilibrium. C) Since the equilibrium constant does not change, nothing happens D) More PCls(g) will be formed. E) Ko -0.17

Explanation / Answer

32)

2 NO2 <—> 2 NO + O2
0.500       0   0 (initial)
0.500-2x   2x   x (at equilibrium)

At equilibrium,
total pressure = 0.500-2x+2x+x = 0.500+x

Given,
total pressure = 0.732
0.500+x = 0.732
x = 0.232

so,
p(NO) = 2x = 2*0.232 = 0.464 atm
Answer: C

Only 1 question at a time please

Related Questions

Navigate

• Browse (All)
• Browse 3
• Subjects

---

---

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