For the reaction 2HI(g) H2(g)+I2(g),Kc= 0.290 at 400 K. If the initial concentra

Question

For the reaction 2HI(g) H2(g)+I2(g),Kc= 0.290 at 400 K. If the initial concentration of HI is 4.0×103M and the initial concentrations of H2, and the initial concentrations of H2, and I2are both 1.50×10–3Mat 400 K, which one of the following statements is correct?

a. The concentrations of HI and I2 will increase as the system is approaching equilibrium.

b. The concentrations of H2 and I2 will increase as the system is approaching equilibrium.

c. The system is at equilibrium.

d. The concentrations of H2 and HI will decrease as the system is approaching equilibrium

e. The concentration of HI will increase as the system is approaching equilibrium.

Explanation / Answer

correct statement :

a) The concentrations of HI and I2 will increase as the system is approaching equilibrium.

2HI(g)   <---------------> H2 (g)    +      I2 (g),

4.0 x 10^-3                   1.50x 10^-3    1.50x 10^-3

Kc = 0.290 M

Qc = [H2][I2] / [HI]^2

     = ( 1.50x 10^-3 )^2 / (4.0x 10^-3)

Qc = 5.625 x 10^-4

Kc = 0.290

here Kc > Qc.

so the reaction shifts forward direction.

so the concentration of H2 and I2 increases. and HI decreases.

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