# First Law of Thermodynamics issue

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

In an experiment to simulate conditions within an automobile engine, 0.155 mol of air at a temperature of 780K and a pressure of 3.20×10

^{6}Pa is contained in a cylinder of volume 310 cm

^{3}. Then 670 J of heat is transferred to the cylinder.

A) If the volume of the cylinder is constant while the heat is added, what is the final temperature of the air? Assume that the air is essentially nitrogen gas.

B) If instead the volume of the cylinder is allowed to increase while the pressure remains constant, find the final temperature of the air.

**2. Relevant equations**

Const P W= pdV Q=nC_{p}dT

Const V W = 0 Q = nC_{v}dT

dU = nCdT

C_{p} = 5/2R

C_{v} = 3/2R

**3. The attempt at a solution**

For part A where Volume is constant, it told me that 670 J of heat is added which would be the Q value for dU. so the overall internal energy is 670 J from that I used the equation dU= nC_{v}(T_{f}-T_{i}) which with values came out too 670 = (.155)(3/2*8.314)(T_{f}-780) which equaled 1126 K. which ended up not being the right answer. I do not know what else to try.

For Part B, I know I need to figure out dU which is Q-W so for this equation it would come out to dU = 670 – pdV or dU = 670 – 3.20E6(V_{f}-3.1E-4m^{3}). but don’t really know where to go from here

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

**2. Relevant equations**

**3. The attempt at a solution**

http://ift.tt/PY7CCI

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