Question

16. According to the following thermochemical equation, if 471.0 g of NO2 is produced, how much heat is released at constant pressure? 2NO(g) + O2(g) → 2NO2(g); ∆H° = –114.4 kJ a) 1.171 × 103 kJ b) 11.17 kJ c) 5.856 × 102 kJ d) 114.4 kJ e) 5.388 × 104 kJ

17. How much heat is liberated at constant pressure if 0.889 g of calcium carbonate reacts with 43.9 mL of 0.756 M hydrochloric acid? CaCO3(s) + 2HCl(aq) → CaCl2(aq) + H2O(l) + CO2(g); ∆H° = –15.2 kJ a) –0.135 kJ b) –13.5 kJ c) –0.252 kJ d) –11.5 kJ e) –0.387 kJ

18. One reaction of iron with hydrochloric acid is represented by the following thermochemical equation. Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g); ∆H°= –87.9 kJ If, in a particular experiment, 8.11 kJ of heat was released at constant pressure, what volume of H2(g), measured at STP, was produced? (R = 0.0821 L • atm/(K • mol)) a) 2.65×102L b) 2.07 L c) 2.26 L d) 2.43×102L e) 22.4 L

19. When 20.0 mL of liquid benzene (C6H6, d = 0.879 g/mL) reacts with 83.4 L of oxygen gas, measured at 1.00 atm pressure and 25°C, 7.35 × 102 kJ of heat is released at constant pressure. What is ∆H° for the following reaction? (R = 0.0821 L • atm/(K • mol)) 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l) a) –3.24 × 103 kJ b) –1.43 × 101 kJ c) –2.02 × 102 kJ d) –3.27 × 103 kJ e) –6.53 × 103 kJ

Show all work and calculations

Answer 1