Consider the following equilibrium: Now suppose a reaction vessel is filled with

Question

Consider the following equilibrium: Now suppose a reaction vessel is filled with 7.52 atm of nitrosyl chloride (NOCI) and 3.36 atm of nitrogen monoxide (NO) at 828. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NOCl tend to rise or fall? fall Is it possible to reverse this tendency by adding Cl2? In other words, if you said the pressure of NOCl will tend to rise, can that be changed to a tendency to fall by adding Cl Similarly, if you said the pressure of NOCl will tend to fall, can that be changed to a tendency to rise by adding Cl? If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl2 needed to reverse it. Round your answer to 2 significant digits. yes no atm

Explanation / Answer

DG0 = - RTlnKp

41*10^3 = - 8.314*1283lnk

Kp = 0.0214

Kp = pNO^2*pCl2/pNOCl^2

as there is no, Cl2 available the equilibrium reaches from forward reaction.

so that, the pressure of NOCl tend to fall . answer : fall

yes , by adding Cl2, it is possible to reverse this tendency.

Kp = pNO^2*pCl2/pNOCl^2

0.0214 = (((3.36+x)^2)*((x/2)))/(7.52-x)^2

x = 0.183

minimum partial pressure of Cl2 required = x/2 = 0.183/2 = 0.092 atm

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

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