Gas laws....

If the question deals with the mass or moles of a substance at a specific temperature and pressure, then use the ideal gas equation:

PV = nRT

A handy variation of the ideal gas equation is PV = mRT / M (where m is mass, and M is molar mass).

If you are dealing with changes in pressure, volume or temperature for a confined gas, then use the combined gas law:

P1V1 / T1 = P2V2 / T2

If T is constant, then it reverts to Boyle's law: P1V1 = P2V2

If P is constant, then it reverts to Charles's law: V1/T1 = V2/T2

If V is constant, then it reverts to Amontons's law: P1/T1 = P2/T2

Note: there is no such gas law as "Gay-Lussac's law" expressed as P1/T1 = P2/T2. That is a myth which has been propagated for years by teachers and even textbook authors, people who should know better. Gay-Lussac investigated the same phenomena as did J. Charles. But Charles didn't publish his work. Gay-Lussac did and gave credit to Charles. In some places it is called the "law of Charles and Gay-Lussac."

Now, back to your question. You're dealing with a confined gas which is changing temperature, pressure and volume. Use the combined gas law.

P1V1/T1 = P2V2/T2

V2 = P1V1T2 / (T1P2)

V2 = 1.01 atm x 3.2L x 233K / 306K / 0.25atm

V2 = 9.8L ................... the answer can only be expressed to two significant digits

A comment about question construction. There was absolutely no need to muddy the water using Fahrenheit temperature and inches of mercury if the writer was asking about the combined gas law. If not careful, it becomes a problem about temperature and pressure conversion and not gases. A rule of thumb which question writers should follow is to test one concept at a time.