1. (a) Based on the information below, determine ΔGrxn (in kJ) for the following reaction: 2A(g) + B(g) → 2C(g).  A → B                  ΔGrxn = 75kJ ½ C →  B             ΔGrxn = 45kJ  C → A                  ΔGrxn = -25kJ Answer ________________ 2. The reaction in the previous question is exothermic. Which of the following statements is true?   A The reaction is spontaneous at all temperatures.   B The reaction is spontaneous at high temperatures.   C The reaction is spontaneous at low temperatures.   D The reaction is not spontaneous at any temperature.

The ΔE of a system that absorbs 184 J of heat from the surroundings and has 42 J of work done on the system is ________ .

Another group performed the combustion of sucrose. Determine the ΔHcombustion (in kJ/mol) of sucrose given the following data obtained by the other group. Combustion Reaction: C12H22O11(s)+12CO2(g)+11H2O(l)   Mole of sucrose: 0.002 mol Ccal of the bomb calorimeter: 7943.1 J/ºC increment T: 1.36 ºC mass of burnt fuse wire: 0.0108 g qwire,surr: 5858 J/g   Express your answer in 2 decimal places. Round your answer to 2 decimal places.

Use data from Appendix attached to calculate ΔS∘rxnΔ�rxn∘ for each of the reactions given. SO2(g)+12O2(g)→SO3(g)SO2(g)+12O2(g)→SO3(g) Express your answer using one decimal place in J/K.

Δ Use the Hess’ Law to calculate DH°(tot) for the [tot] reaction from the DH°’s given: [tot]            2Fe2O3(s) + 3C(s) ® 4Fe(s) + 3CO2(g)   ΔH°(tot) = ________? kJ [1]              4Fe(s) + 3O2(g) ® 2Fe2O3(s)                ΔH°1 = –824 kJ      [2]              C(s) + O2(g) ® CO2(g)                          ΔH°3 = –394 kJ [tot] = ___×[1] ___×[2]          add up equations [1] and [2] scaled by the factors you chose, and cancel any formulas that are the same on both sides: ______________ --> ______________ same as [tot] after cancelling? ___  if “Yes”, scale the enthalpies ΔH°1,2 by the factors you chose for their equations, and combine for the ΔH°(tot) =  ___×ΔH°1 ___×ΔH°2 = ______kJ

#2 For each reaction, find the value of ΔSo. Report the value with the appropriate sign. (a)   3 NO2(g) + H2O(l) →2 HNO3(l) + NO(g) =____J/K   (b)    N2(g) + 3 F2(g) →2 NF3(g) =____J/K   (c)    C6H12O6(s) + 6 O2(g) →6 CO2(g) + 6 H2O(g) =____J/K

Given the following data: N2(g) + O2(g) → 2NO(g) ΔH = +180.6 kJ 2CO2(g) + N2(g) → 2CO(g) + 2NO(g) ΔH = 746.6 kJ Find the ΔH of the following reaction: 2CO2(g) → 2CO(g) + O2(g)

A potential chemical reaction at 25.0 °C has a ΔHrxn of 136.1 kJ and a ΔSrxn of -403.9 J/K. What is the ΔGrxn in kJ.  (Enter answer to 3 significant figures and include no units in your answer)