Answer:
Exothermic
1771 g
Explanation:
Step 1: Write the balanced thermochemical equation
2 S(s) + 3 O₂(g) ⇒ 2 SO₃(g) ΔH° = -791.4 kJ
Since ΔH° < 0, the reaction is exothermic.
Step 2: Calculate the moles of SO₃ produced when 8753 kJ of energy are released
According to the thermochemical equation, -791.4 kJ are released every 2 moles of SO₃ that are formed.
-8753 kJ × 2 mol/(-791.4 kJ) = 22.12 mol
Step 3: Calculate the mass corresponding to 22.12 moles of SO₃
The molar mass of SO₃ is 80.06 g/mol.
22.12 mol × 80.06 g/mol = 1771 g
