If 12 g gives you n = 0.211 mol, then how many moles does 14.5 g give you? Once you have the new n value you can solve for the pressure in the second case.
I would personally take the following approach to the problem, especially since the gas constant is not given in the question and I can't remember it for mmHg...
now,
PV = nRT, so let's say for the first case P1V1 = n1RT1
rearrange: (P1V1)/(n1T1) = R
Similarly, for the second case:
(P2V2)/(n2T2) = R
So, since both equal R...
(P1V1)/(n1T1) = (P2V2)/(n2T2)
Since V1 = V2, we simplify to...
P1/(n1T1) = P2/(n2T2) <- Equation (1)
Considering that n = m/mr (m = mass; mr = molecular mass
It follows that...
n1 = m1/mr and n2 = m2/mr
Substitute for n1 and n2 in equation (1)...
(P1mr)/(m1T1) = (P2mr)/(m2T2)
mr's cancel out...
P1/(m1T1) = P2/(m2T2)
Rearrange:
P2 = (P1m2T2)/(m1T1)
All the values for the terms on the right hand side are given in the question, P2 is the only unknown. Plug in the numbers and you have your answer.