1. Suppose that 25 J of heat is added to one mole of an ideal gas. The gas expands at a constant pressure of 2.62 x 10^4 pascals while changing its volume rom 4.97 x 10^-4 m^3 to 7.02 x 10^-4 m^3. Calculate C_p and express in Joule / (mole * Celsius) 2. Relevant equations Q = C_p*n*(delta T) P(Delta V) = nR(Delta T) 3. Attempt at solution 25 J = C_p (1 mole) (Delta T) Delta T = .64632 Kelvin Delta T = -272.35 Celsius 25 J = C_p (1 mole) ( .272.35 Celsius) C_p = -.0918 J / (mole*Celsius) 4. Question: I inputted the answer into the online system as +.0918 J / (mole*celsius) However, it is telling me that I am wrong. Could there be a negative molar specific heat capacity? That doesn't make too much sense to me because shouldn't the molar specific heat raise the temperature? Or did I do some stupid mistake with units/wrong equations?