Given the equation S(s)+ O₂(g)$\to$ SO₂(g),$\Delta$H = -296 kJ,which of the following statement(s)is (are)true? I.The reaction is exothermic. II.When 0.500 mole sulfur is reacted,148 kJ of energy is released. III.When 32.0 g of sulfur are burned,2.96 $\times$ 10⁵ J of energy is released.

Question

Quizplus · Accepted Answer

The reaction is exothermic because the enthalpy change is negative. When 0.500 mole of sulfur is reacted, half of 296 kJ (i.e., 148 kJ) is released. Burning 32.0 g of sulfur (1 mole) releases 296 kJ, which is equivalent to 2.96 × 10^5 J.

Given the Equation S(s)+ O2(g) →\to→ SO2(g) Δ\DeltaΔ H = -296 KJ,which of the Following Statement(s)is (Are)true? I

Given the Equation S(s)+ O₂(g) $\to$ SO₂(g) $\Delta$ H = -296 KJ,which of the Following Statement(s)is (Are)true? I