Consider the following equilibrium: 2NOCl (g) 2NO (g) + Cl_2 (g) Delta G^0 = 41.

Question

Consider the following equilibrium: 2NOCl (g) 2NO (g) + Cl_2 (g) Delta G^0 = 41. kJ Now suppose a reaction vessel is filled with 7.99 atm of nitrosyl chloride (NOCl) and 3.24 atm of nitrogen monoxide (NO) at 993. degree C. Answer the following questions about this system: Under these conditions, will the pressure of NOCl tend to rise or fall? Is it possible to reverse this tendency by adding Cl_2? 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_2? Similarly, if you said the pressure of NOCl will tend to fall, can that be changed to a tendency to rise by adding Cl_2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of Cl_2 needed to reverse it. Round your answer to 2 significant digits.

Explanation / Answer

P-NOCl = 7.99

P-NO = 3.24

Qp = (7.99^2)/(3.24) = 19.7

Clearly, this favours reactants, so expect NOCl to incrase / RISE in pressure

b)

Adding more Cl2 will favour more NOCl formation

c)

N/A since no need to calculate CL2

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

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