1. A. Products because K>1
    B. Reactants because K<1
    C. Products because K>1

2. First, find change in enthalpy:
    DH(reaction) = DH(reactants) -  DH(products) = [6(-393.5 kJ/mol) + 6 (-285.8 kJ/mol)] - (-1274.4 kJ/mol) = -2801 kJ/mol
   Second, find heat release from the combustion of 1 gram:
    1 g x 1 mole/180 grams x -2801 kJ/mole x 1 kcal/4.184 kJ = -3.75 kcal/g

3.  A. Endothermic (this reaction is the opposite of the exothermic one in question 2).
     B. More product
     C.  2 g O₂ x 1 mole O₂/32 g x 1 mole C₆H₁₂O₆/6 mole O₂ x 2801 kJ/mol C₆H₁₂O₆ = 29.2 kJ/mol
     D. DS(reaction) = DS(reactants) -  DS(products) = [212 J/molK + (6)205 J/molK] - [(6)214 J/molK + (6)70 J/molK] =  -262 J/molK
        so entropy decreases
     E. Entropy must increase somewhere