- 00 mol of Cu at 500 °C was placed in 200 g of water at 25.00 °C. This system was thermally insulated. A.) (10) What is the final temperature of the system? B) (15) What was ∆H for the Cu and for the water?
- (25 pts) True of False (if false, explain why)
- _______ ∆U is usually straightforward to measure in a bomb calorimeter.
- _______ If there are no phase changes, a plot of CP vs T can be integrated to yield the entropy change for a substance.
- _______ The entropy of all substances appear to extrapolate to 0 at 0 K.
- _______ The entropy change for boiling is roughly constant.
- _______ ∆S must be calculated over a reversible path.
- Liquid water, 36 g initially at 50 °C was put into a large freezer at -10°C. The water didn’t freeze until -10 °C (it was supercooled). A) (15 pts) What is ∆S for the water for this process? B) (10 pts) What is the total ∆S for the overall system and is the process spontaneous?
- (15 pts) One mol of an ideal monoatomic gas is expanded from 300 K and 10 bar to 350 K and 5 bar. Calculate ∆U, ∆H, and ∆S for this process. Is this a spontaneous process? (10 pts) Given S as a function of T and P, show that dS(T,P) = (CP/T) dT – (∂V/∂T)PdP
CV (monoatomic) = (3/2) R, CP (monoatomic) = (5/2) R,
R = 8.314 J/K/mol = 0.08205 L atm/K/mol
Cp (H2O, liquid) = 75.3 J/K mol, Cp (H2O, ice) = 37.2 J/K mol ∆Hf = 334 J/mol.
- (0 pts)
Who was the “Man in Black?” ______________________
Where was the California country music capital? ______________________