stoichiometry_and_heat_capacity

Stoichiometry and Heat Capacity 1. Calculate the heat evolved (kJ) for the reaction in which 9.00 g of C 6 H 12 O 6 is fermented to form ethyl alcohol (Atomic weights: C = 12.01, H = 1.008, O = 16). C 6 H 12 O 6 (s) 2 C 2 H 5 OH(l) + CO 2 (g) ∆ H o = -67.0 kJ 2. Calculate the heat energy (kJ) released when 15 g of Fe 3 O 4 reacts with excess Al according to the following reaction. (Atomic weights: Fe = 55.85, Al = 26.98, O = 16.00). 3 Fe 3 O 4 (s) + 8 Al(s) 4 Al 2 O 3 (s) + 9 Fe(s) ∆ H o = -3347.6 kJ 3. What quantity of heat is liberated by a reaction that produces 50.0 g of SO 2 in the following reaction? (Atomic weights: Ni = 58.69, O = 16.00, S = 32.06). 2 NiS(s) + 3 O 2 (g) 2 NiO + 2 SO 2 (g) ∆ H o = -936.2 kJ 4. A 25.0 g piece of copper at 25.0 o C is put into an insulated vessel containing 100 g of water at 40.0 o C. What will be the final temperature ( o C) of the water? The specific heat of copper and water are 0.385 J/g o C and 4.18 J/g o C respectively. 5. How much heat energy (kJ) must be supplied to heat 400.0 g of isopropyl alcohol from 20.0 o C to 60.0 o C in a stainless steel vessel weighing 550.0 g. The specific heat of isopropyl alcohol and stainless steel are 2.58 J/g o C and 0.51 J/g o C respectively. 6. A sheet of 10.0 g of copper at 22.0 o C is placed on a 20.0 g sheet of aluminum at 75.0 o C. What is the final temperature of the two metals assuming that no heat is lost to the surroundings. The specific heats of copper and aluminum are 0.385 J/g o C and 0.900 J/g o C respectively.