Answer:
D) cutting the concentrations of both NOBr and NO in half
Explanation:
The equilibrium reaction given in the question is as follows -
2NOBr ( g ) ↔ 2NO ( g ) + Br₂ ( g )
The equilibrium constant for the above reaction can be written as -
K = [ NO ]² [ Br₂ ] / [ NOBr ] ²
Therefore from the condition given in the question , the changes that will not affect the equilibrium will be , reducing the concentration of both NOBr and NO to half ,
Hence ,
the new concentrations are as follows -
[ NoBr ] ' = 1/2 [ NoBr ]
[ NO ] ' = 1/2 [ NO ]
Hence the new equilibrium constant equation can be written as -
K ' = [ NO ] ' ² [ Br₂ ] / [ NOBr ] ' ²
Substituting the new concentration terms ,
K ' = 1/2 [ NO ] ² [ Br₂ ] / 1/2 [ NoBr ] ²
K ' = 1/4 [ NO ] ² [ Br₂ ] / 1/4 [ NoBr ] ²
The value of 1 / 4 in the numerator and the denominator is cancelled -
K ' = [ NO ] ² [ Br₂ ] / [ NoBr ] ²
Hence ,
K' = K
