I can't tell you the multiple choice answer, but that should not matter...
Since
Recall that an equilibrium constant for the reaction
$aA + bB -> cC + dD$
is
$K_(eq) = ([C]^c[D]^d)/([A]^a[B]^b)$ ,where
$a,b,c,d$ are the stoichiometric coefficients of$A,B,C,D$ , respectively, and$[" "]$ indicates molar concentration.
If an equilibrium constant is small, i.e.
$K_(eq) < 1$ ,then that means there are more reactants than products before the equilibrium is disturbed.
(Note that in principle, the actual size of
$K_(eq)$ does not affect which direction the equilibrium shifts given a certain induced stress.)
Adding more reactants initially decreases the reaction quotient
Since
That means it will shift to consume more reactants to generate more products.