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1. Calculate the work done (in joules) for the given cyclic process.

1.	300	2.	200
3.	400	4.	600

2. Which of the following parameters are path functions?
(A) \( q+w \)
(B) \(q\)
(C) \(w\)
(D) \(H-TS \)
1. (B) and (C)
2. (B), (C) and (D) 
3. (A) and (D) 
4. (A), (B) and (C) 

3. Consider the following reaction:
\(\mathrm{A}_2(\mathrm{~g})+3 \mathrm{~B}_2(\mathrm{~g}) \rightarrow 2 \mathrm{AB}_3(\mathrm{~g})\)
If at 300K, the enthalpy change for the above reaction is +15 kJ, then the internal energy change is:

1.	19.98 K J	2.	200 J
3.	1999 J	4.	1.9988 kJ

4. The specific heat of tungsten is 0.03 cal/g-°C. If a 50 gram sample of tungsten absorbs 100 calories of heat, the change in temperature of the sample will be:
1. 76 °C
2. 55 °C
3. 67 °C
4. 62 °C

5. Work done during reversible isothermal expansion of one mole of hydrogen gas at 25°C from a pressure of 20 atmospheres to a pressure of 10 atmospheres is:
(Given: R = 2.0 cal K^–1 mol^–1)

1.	–413.14 calories	2.	413.14 calories
3.	100 calories	4.	0 calorie

6. Calculate the standard enthalpy of reaction for the following reaction using the given enthalpies of reaction:
\(3 \mathrm{Co}(s)+2 \mathrm{O}_2(g) \rightarrow \mathrm{Co}_3 \mathrm{O}_4(s)\)
Given:
\(2 \mathrm{Co}(s)+\mathrm{O}_2(g) \rightarrow 2 \mathrm{CoO}(s) ; \Delta H_1^{\circ}=-475.8 \mathrm{~kJ}\)
\(6 \mathrm{CoO}(s)+\mathrm{O}_2(g) \rightarrow 2 \mathrm{Co}_3 \mathrm{O}_4(s) ; \Delta H_2^{\circ}=-355.0 \mathrm{~kJ}\)
1. \(-891.2 \mathrm{~kJ}\)
2. \(-120.8 \mathrm{~kJ}\)
3. \(+891.2 \mathrm{~kJ}\)
4. \(-830.8 \mathrm{~kJ}\)

7. Consider an imaginary reaction, \(X \longrightarrow Y\) that occurs in three steps:
\(X \longrightarrow A, ~~\Delta H=-q_1 ;\\ B \longrightarrow A, ~~\Delta H=-q_2 ;\\ B \longrightarrow Y,~~ \Delta H=-q_3;\)
If Hess' law is applicable, then the heat of the reaction \((X \longrightarrow Y)\) is:
1. \(q_1-q_2+q_3\)
2. \(q_2-q_3-q_1\)
3. \(q_1-q_2-q_3\)
4. \(q_3-q_2-q_1\)

8. Calculate \(\Delta S^\circ \) in (J/K) for the reaction:
\(2 \mathrm {Al} \text {(s)} + 3 \mathrm {MgO} \text {(s)} \rightarrow 3 \mathrm {Mg}\text {(s)} + \mathrm {Al_2O_3} \text {(s)}\)
(Given are the following standard molar entropies measured at \(25^\circ \text {C}\) and 1 atm pressure)

\(​\mathrm{Al} \)(s) = 28.0 J/K

\(\mathrm {MgO} \text {(s)}\) = 27.0 J/K

\(\mathrm {Mg}\text {(s)}\) = 33.0 J/K

\(\mathrm {Al_2O_3} \text {(s)}\) = 51.0 J/K

1. -29.0 J/K
2. -13.0 J/K
3. +13.0 J/K
4. +69.0 J/K

9. A certain reaction has a \(\Delta H^{\circ}=-43.2 \mathrm{~kJ} \mathrm{~mol}^{-1} \) and an entropy change \(\Delta S^\circ\) of \(+22.0 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}.\) What is the value of \( \Delta G^\circ\) at \(800~^\circ C?\)
1. \(-66.8 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
2. \(+21.2 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
3. \(-21.2 \mathrm{~kJ} \mathrm{~mol}^{-1}\)
4. \(-2365 \mathrm{~kJ} \mathrm{~mol}^{-1}\)

10. Which of the following statements is true about an isolated system?
1. Heat passes into or out of the system.
2. Matter enters or leaves the system.
3. Work can be done on the system.
4. None of the above.