Chemical Equilibrium

I am given this problem for my General Chemistry II class, and am can't figure it out. I've done quite a few of these and they've all been extremely easy, but I think I'm missing something with this one.

Consider the following reaction:
A (g) <=> 2B (g)
Find the equilibrium partial pressures of A and  B for each of the following different values of Kp. Assume that the initial partial pressure of rm B in each case is 1.0  atm and that the initial partial pressure of A is 0.0 atm. Make any appropriate simplifying assumptions.

It then gives me Kc (yes, Kconcentration) and no temperature is given anywhere for me to convert it to Kp with.

Kc = 1.2
pA = ?
pB = ?

Initially I set up an ICE chart (this may be formatted incorrectly...):
_______________A <=> 2B
Initial         0      1.0
Change         -x      +2x
Equilibrium    -x      1.0+2x


And then used the eq. values in the K expression Kp=[B]^2 / [A] and was unable to produce an acceptable result. I then tried flipping the equilibrium equation and using the inverse of 1.2 and placing those values in the chart to no avail.

There is no other information given anywhere on the page.

What am I doing wrong, please help! 
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OP here, disregard this thread. I made an incredibly dumb mistake of misplacing a decimal point.

fuck

Your ICE is set up wrong.  Think through it logically:  you have it set up so that the partial pressure of A is going to be negative.  How is that going to work?

I think the algebra is going to turn out right (assuming you end up with a x<0, but it's set up really oddly, so that might be your problem.