Given the equation S(s) + O₂(g) $\rightarrow$ SO₂(g) , $\Delta$ H = -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

Given the equation S(s) + O₂(g)

\rightarrow

SO₂(g) ,

\Delta

H = -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.

Quizplus · Accepted Answer

The Answer of Given the equation S(s) + O₂(g) $\rightarrow$SO₂(g), $\Delta$H = -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.

Given the Equation S(s) + O2(g) →\rightarrow→ SO2(g) Δ\DeltaΔ H = -296 KJ, Which of the Following Statements Is(are)

Given the Equation S(s) + O₂(g) $\rightarrow$ SO₂(g) $\Delta$ H = -296 KJ, Which of the Following Statements Is(are)