What quantity,in moles,of oxygen is consumed when 717.4 kJ of energy is evolved from the combustion of a mixture of H₂(g) and O₂(g) ?
H₂(g) +
O₂(g) → H₂O(l) ; ΔH° = -285.8 kJ

Question

What quantity,in moles,of oxygen is consumed when 717.4 kJ of energy is evolved from the combustion of a mixture of H₂(g) and O₂(g) ?
H₂(g) +

What quantity,in moles,of oxygen is consumed when 717.4 kJ of energy is evolved from the combustion of a mixture of H<sub>2</sub>(g) and O<sub>2</sub>(g) ? H<sub>2</sub>(g) + O<sub>2</sub>(g) → H<sub>2</sub>O(l) ; ΔH° = -285.8 kJ A) 1.255 mol B) 2.519482 mol C) 0.1991 mol D) 1.755 mol E) 0.7559321 mol

O₂(g) → H₂O(l) ; ΔH° = -285.8 kJ

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The Answer of What quantity,in moles,of oxygen is consumed when 717.4 kJ of energy is evolved from the combustion of a mixture of H₂(g)and O₂(g)? H₂(g)+ O₂(g)→ H₂O(l); ΔH° = -285.8 kJ A)1.255 mol B)2.519482 mol C)0.1991 mol D)1.755 mol E)0.7559321 mol

What Quantity,in Moles,of Oxygen Is Consumed When 717