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2NO (g) + 2Cl2 = 2NOCl2 (g) given: Kp = 65000, what is themolarity of NOCl2 when the system is at equilibrium given that thepressure of NOCl2 = 8.9atm, partial pressure of NO = 0.35atm, andpartial pressure of Cl2 = 0.10atm

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Related questions

In a container, the partial pressure of NOCl is initially 0.3915 atm at a given temperature. The chemical equation which describes the reaction is:

2NO (g) + Cl2(g) 2NOCl(g)


At equilibrium analysis shows the partial pressure of NO is 0.102 atm.
a) Which direction did the reaction proceed to establish (reach) equilibrium?

b) What is the partial pressure of NOCl which reacted in order for the partial pressure of NO to be 0.102 atm?

c) What is the partial pressure of Cl2 at equilibrium?

d) What is the partial pressure of NOCl at equilibrium?

e) What is the magnitude of KP for the equation above?

In a container, the partial pressure of NOCl is initially 0.3465 atm at a given temperature. The chemical equation which describes the reaction is: 2NO (g) + Cl2(g) 2NOCl(g) At equilibrium analysis shows the partial pressure of NO is 0.093 atm. What is the partial pressure of NOCl which reacted in order for the partial pressure of NO to be at 0.093 atm? What is the magnitude of Kp?

A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine as shown by the reaction below: 

 

When the system comes to equilibrium at 425 °C, the partial pressure of HI = 0.708 atm and partial pressure of H2 = partial pressure of I2. What is the equilibrium constant, Kp, value at this temperature?

 

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