First off, thanks for the help on the other problems...

Question

For the reaction, A(g) + 2 B(g) <==> 2 C(g), Kc = 1 x 10-10 at 25°C. Which of the following statements is true?

1. Delta n = +1
2. The concentration of the products is greater than the concentration of the reactants.
3. The reaction is favored in the reverse direction.
4. The value of Kp will be larger than the value for Kc.

1 is false because delta n = -1.
4 is false because Kp = 4.087e-12 (which is smaller than Kc)

I believe it is not favored in the reverse direction... but then how would I know if the concentrations of the products are greater than that of the reacants?

1 is false.
2 is false. K_c=(C)²/(A)*(B)².
With K = 10^-10, the only way to get a number smaller than 1 is for the products to be small and the reactants to be large.
4 is false as you have said.
3 is correct. Same reasoning as 2. Products are small and reactants are large which means the reactants are favored and that means the reaction goes in the reverse direction (ALTHOUGH, with a double arrow, I wonder exactly what is meant by "the reverse direction--technically I don't know that there is a reverse direction). The answer would have been better stated as "the left side is favored over the right side." The intent of the problem, however, is for the answer to be 3.