3. (2) Does the entropy of the surroundings always increase for spontaneous processes? Explain. (b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ASur? (c) During a certain reversible process, the surroundings undergo an entropy change, - 75J/K. What is the entropy change of the system for this process?

When dry ice (solid CO 2) sublimates, its entropy(A) increases(B) decreases(C) does not change(D) could either increase or decrease, depending on other factors

5-For the reaction, A+B C, AH-+30 kJ; AS°=+50 J/K.Therefore the reaction is: (a) spontaneous at all temperatures. (b) nonspontaneous at all temperatures. (d) irreversible at all temperatures (c) reversible at all temperatures 6- How much heat is necessary to convert 2mol of water at( 50°C) to steam at 150°C?The molar heat capacity of liquid water and steam are 75.3 J/mol. K and 36.4 J/mol. K respectively. The heat of vaporization 40.7 KJ/mol. a-81400J 7- From the reactions: b-82.337KJ c-753J d-3641 e- none of them Cgraphia +2H2(g) → CHA(R) AH = -79.9KJ C(graphia + 2Cl2(g) → CCla AH = -139KJ H 20 + Cl₂00) → HCL) AH-92.3KJ 202) calculate AH, for the reaction CH ACE +4Cl2) a- (-615.1KJ) c-(-428.3KJ) 4HCI+CCI b-(-311.2KJ) d- none of them

Methanol is relatively inexpensive to produce. Much consideration has been given to using it as a precursor to other fuels such as methane, which could be obtained by the decomposition of the alcohol. CH3OH(l) -> CH4(g) + 1/2 O2(g) (a) What are the sign and magnitude of the entropy change for the reaction? Does the sign of Δ

An endothermic reaction proceeds spontaneously. What can you deduce about the sign of Delta S for this process? Explain.