Which statement best describes the driving force for the reaction: BCI3 + O(CH2CH3)2 → CI3BO(CH2CH3)2 An electron pair is donated from the LUMO of O(CH2CH3)2 to the HOMO of BCI3 An electron pair is donated from the HOMO of O(CH2CH3)2 to the LUMO of BCI3 There is an increase in entropy for the reaction. There is a decrease in entropy for the reaction.

1. Calculate AHrxn° for the reaction: 2 N₂(g) + 5 O₂(g) → 2 N₂O5(g) from the following data: N₂O5(g) + H₂O(l) → 2 HNO3(1) N₂(g) + 3 O₂(g) + H₂(g) → 2 HNO3(1) 2 H₂(g) + O₂(g) → 2 H₂O(l) AHrxn° = -76.6 kJ AHrxn° = -348.2 kJ AHrxn° = -671.6 kJ

Calculate the standard free energy for the reaction (you may use any valid technique - there may be more than one way to do a question like this): Al2O3(s)) + 3 H2(g) → 2 Al(s) + 3 H2O(g)

Which has lower entropy? CO2(g) or CH4(g)?

The standard reaction free energy AGO = − 1378. kJ for this reaction: 2 CH3OH(g) + 3O₂(g) →2 CO₂(g) + 4H₂O(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. 2 4 ²-CH₂OH(g) + O₂(g) → ²-CO₂(g) + H₂O(g) 3 2 3 reaction 3 -- CO₂(g) + H₂O(g) + H₂O(g) → 2 2CO₂(g) + 4H₂O(g) 1 2 3 CH₂OH(g) + ²/0₂(g) 4 2 2CH₂OH(g) + 30₂ (8) 2 0 46° kJ KJ kJ x10 Ś

Chp 19 #28 & # 30

A 0.582-g sample of Mg reacts with excess 1.0 M HCl (60.0 mL) according to the procedure used in this experiment. The initial and final temperatures were 24°C and 68°C. What is the ∆H of the reaction per mole of magnesium? Assume that the specific heat capacity for the solution is 4.187 J/oC∙g and that the density of the 1.0 M HCl is 1.00 g/mL. (Hints: the magnesium contributes to the mass of the solution; take care with your sig figs.) (answer: - 4.7 × 102 kJ/mol)Show your solution to this problem in the space below. It is your solution which will be graded.

a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) =  -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l)  b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?

The following reactions (in the left column) have been observed to be spontaneous. For each reaction decide which OA is stronger and which RA is stronger in the right column. An example is shown.