Chemistry, 22.05.2020 11:58 JOEREACH

Consider the following reactions. (Note: (s) = solid, (l) = liquid, and (g) = gas.)
Mg(s) + ½O2(g) → MgO(s) + 146 kcal/mole
H2(g) + ½O2(g) → H2O(g), ΔH = -57.82 kcal/mole
What type of reaction is represented by the previous two examples?
A: exothermic
B: endothermic

Answers: 3

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Consider the following reactions. (Note: (s) = solid, (l) = liquid, and (g) = gas.)
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Consider the following reactions. (Note: (s) = solid, (l) = liquid, and (g) = gas.) Mg(s) + ½O2(g) → MgO(s) + 146 kcal/mole H2(g) + ½O2(g) → H2O(g), ΔH = -57.82 kcal/mole What type of reaction is represented by the previous two examples? A: exothermic B: endothermic

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Consider the following reactions. (Note: (s) = solid, (l) = liquid, and (g) = gas.)
Mg(s) + ½O2(g) → MgO(s) + 146 kcal/mole
H2(g) + ½O2(g) → H2O(g), ΔH = -57.82 kcal/mole
What type of reaction is represented by the previous two examples?
A: exothermic
B: endothermic