**1. The problem statement, all variables and given/known data**

A cylinder fitted with a movable piston contains ideal gas at 27C, pressure .5 x 10^5 Pa, and volume 1.25 m^3. What will be the final temperature if the gas is compressed to .8 m^3 and the pressure rises to .82 x 10^5 Pa.

A) 125 C

B) 154 C

C) 246 C

D) 67.7 C

E) 41.8 C

**2. Relevant equations**

P1V1/T1=P2V2/T2

**3. The attempt at a solution**

I thought this problem was going to be pretty simple. (.5 x 10^5 Pa x 1.25 m^3)/27 = (.82 x 10^5 Pa x .8 m^3)/T2. I keep getting T2 is equal to 28.3392. Is there something I’m missing? It seems like the pressure/volume ratio doesn’t change that drastically so the temperatures would be close but the closest answer is at ~15 C increase. Any help is appreciated.

http://ift.tt/1k3pmXj