1. Calculate the entropy change for the system, the thermal surroundings, and the total entropy change for one mole of ice melting at +5^oC. The enthalpy change for melting ice is 6.03 kJ/mol.

2. Calculate the D_rH^o and D_rS^o at 25 C for the reaction:

3H2(g) + CO(g) = CH4(g) + H2O(g)

3. Starting with the first and second law and efficiency defined as w/qhot, derive the Carnot efficiency equation for a heat engine.

4. Calculate the DfH, and S of CH4(g) at 0.0035 atm pressure assuming it behaves as an ideal gas.

5. Derive the equation:

DS = R ln(p₁ /p₂)

For the irreversible isothermal expansion of an ideal gas from p₁ to p₂.

6. Calculate q, w, DU, DH, and DS for the reversible isothermal expansion of 1 mole of N₂ from 2.5 bar to 0.75 bar.

7. Calculate q, w, DU, DH, and DS for the conversion of 2 mol of water to 2 mol of steam at 100 C and 1 bar. The heat of vaporization of water is 2260 J/g.

8. Derive the equation:

C_p ln(T₂/T₁) = R ln(p₂/p₁)

Starting with the SECOND LAW of thermodynamics.

1. For a reversible, isothermal expansion of an ideal gas, which of the following equations is FALSE?

a) dU=0 b) dq=-dw c) dS= dq/T d) dT=0 e) dS=dU/T

2. Consider the signs of q,w,U,T, and S for a reversible, adiabatic expansion of an ideal gas. Which of the following is correct?

a) dq=0 dw<0 dU=0 dT<0 dS>0 b) dq=0 dw>0 dU<0 dT>0 dS<0 c) dq>0 dw<0 dU<0 dT<0 dS>0

d) dq<0 dw<0 dU<0 dT<0 dS<0 e) dq=0 dw<0 dU<0 dT<0 dS=0

3. For the reversible freezing of water at 0 C; which of the following equations is NOT true?

a) DS = DH/T b) DSTotal =0 c) DG =0 d) dq=0 e) dT=0

4. The vaporization of HCl(l) at its normal boiling point of -85 C is accompanied by an enthalpy of vaporization of 16.15 kJ/mol. The standard entropy of vaporization of HCl is _____J/K.

a) -190 b) .0859 c) 85.9 d) 190

5. For the spontaneous process at 1 atm: ice (5 C) => water (5 C) select the correct set of signs for the entropies.

DSsystem DSsurroundings DStotal

a) + - 0

b) - + 0

c) + - +

d) + + +

6. 600 J of heat is irreversibly transferred from a hot object at 600 K to a cold object at 300 K. What is the total change in entropy of the process.

a) 1 J/K b) 1 J c) 0 d) 300 J e) none of these