This question relates to partial pressures. I beleive I have to use an ice table

Question

This question relates to partial pressures. I beleive I have to use an ice table but I cant seem to figure this out.

For a particular reaction at equilibrium, the pressure of the bromine is 2.0 atm at 25°C. The total pressure in the vessel at equilibrium is 10.0 atm. The balanced chemical equation is:

2NOBr (g) <-- --> 2NO (g) + Br2 (g)

What is the value of Kp for the reaction?

This question relates to partial pressures. I beleive I have to use an ice table but I cant seem to figure this out.

For a particular reaction at equilibrium, the pressure of the bromine is 2.0 atm at 25°C. The total pressure in the vessel at equilibrium is 10.0 atm. The balanced chemical equation is:

2NOBr (g) <-- --> 2NO (g) + Br2 (g)

Explanation / Answer

2 NOBr (g) <-------------> 2 NO (g)   + Br2 (g)

y                                           0               0

y - 2x                                     2x               x

At equilibrium :

pressure of Br2 = x = 2.0 atm

total pressure = 10.0 atm

y - 2x + 2x + x = 10

y + x = 10

y + 2 = 10

y = 8

pressure of NOBr = y - 2x = 8 - 4 = 4 atm

pressure of NO = 2x = 4 atm

Kp = P2NO x Pbr2 / P2NOBr

      = 4^2 x 2 / 4^2

     = 2

Kp = 2.0

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