The correct option is A Reaction will proceed in forward direction until equilibrium is established.
Given, nH2=0.22, nI2=0.2, nHI=0.66V=1L
∴[H2]=0.22,[I2]=0.22,[HI]=0.66
The concentration given in question are not necessarily the equilibrium concentrations.
Calculating reaction quotient Qc from these concentrations :
The reaction is
H2+I2⇌2HI
For this reaction, Qc=[HI]2[H2][I2]
putting the value,
Qc=(0.66)2(0.22)(0.22)
Qc=9.0 but Kc=49 (Given), which is greater than Qc
i.e. Kc>Qc
Hence, the reaction will move in forward direction.