Write the balanced formation reaction of 1-propanol, CH_3CH_2CH_2OH(l) or C_3H_3O(l). Make sure to include (s), (l) or (g) for each species. Consider the calorimetry equation q_rxn = -C delta T a. In a bomb (closed) calorimeter the measured q_rxn = C delta T equals delta H/delta U a. For an endothermic reaction T of the calorimeter+ content increases/decreases c. Bond energies are always defined with: negative/positive values d. The standard enthalpy of formation of a compound is: always negative can be positive or negative/always positive The molar heat capacity of a compound is empirically represented as C_p, m = A + BT + CT^-2 Derive the equation for delta H_m when the temperature rises from T_1 to T_2. Remember delta H = integral CdT and integral x^a dx = 1/a + 1 x^a + 1