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 7.20 atm of chlorine (Cl 2) and 7.66 atm of nitrosyl chloride (NOCI) at 1140·°C. Answer the following questions about this system rise fall Under these conditions, will the pressure of CI2 tend to rise or fall? ×10 Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl2 will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl 2 will tend to fall, can that be changed to a tendency to rise by adding NO? yes no If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. Round your answer to 2 significant digits atim

Explanation / Answer

i)

Answer

Raise

Explanation

G° = -RTlnK

logK= -G°/2.303RT

= -(-41000J/2.303×8.314(J/K mol)×1413.15K)

= 1.515

K = 1×10^1.515=32.73

Q= (7.66atm)^2/(0)^2 × 7.20

Q = infinity

Q> K

So, the reaction is reverse side

So, pressure of Cl2 tend to raise

ii)

Answer

Yes

Explanation

when, Q < K

the reaction is forward side

So, if we add NO such that the condition Q<K is reversed then the reaction will move to forward direction and presssure of Cl2 tend to decrease

iii)

Answer

Minimum NO pressure required = 0.50atm

Explanation

When ,

Q = K

(7.66atm)^2/((p(NO))^2× 7.20atm)= 32.73atm^-1

(p(NO))^2 = (7.66atm)^2/(32.73atm^-1×7.20atm)

(p(NO))^2 = 0.249atm^2

p(NO) = 0.50atm

  

  

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