Given the equation S(s) + O₂(g) → SO₂(g) , ΔH = -296 kJ, which of the following statements is(are) true?
I. The reaction is exothermic.
II. When 0.500 mol of sulfur is reacted, 148 kJ of energy is released.
III. When 32.0 g of sulfur is burned, 2.96 × 10⁵ J of energy is released.

Question

Quizplus · Accepted Answer

The reaction is exothermic because ΔH is negative, indicating energy is released. For II, since ΔH = -296 kJ per mole of sulfur, 0.500 mol would release half of that energy, or -148 kJ. For III, 32.0 g of sulfur is equivalent to 1 mol (given sulfur's molar mass is approximately 32 g/mol), so the energy released would be -296 kJ, or -2.96 × 10^5 J, matching the statement.

Given the Equation S(s) + O2(g) → SO2(g), ΔH =

Given the Equation S(s) + O₂(g) → SO₂(g), ΔH =