"The H for a reaction has been determined to be -315.69 kJmol and its S is 25.32 JmolK. Assume these values do not change significantly with temperature. As temperature is increased, the equilibrium constant, K_eq will approach what minimum value?"

I have tried using lnKeq= -DeltaH/RT + DeltaS/R . Both times I have gotten no where, and I know these answers are wrong. I know I need to consider what happens to the terms that define the relationship between the equilibrium constant and temperature when the temperature approaches infinity, but in this case I though that Delta H would become dominant. I thought then, if that wasn't the case I would set to 0 and solve in that manner, but my original is negative, making the overall problem positive, and a very large number. So when I calculated the Keq, my calculator wouldn't even work. I know I need to find the upper limit for Keq, and to do that I need to solve for Keq, but I'm doing something wrong. If someone could do a step by step process, I may be able to finally pinpoint if I'm doing the math wrong, or if my understanding of the concept is wrong, I would greatly appreciate it.