?The following equation shows the conversion of aluminum oxide (from the ore bauxite) to

Chapter 7, Problem 7.4

(choose chapter or problem)

The following equation shows the conversion of aluminum oxide (from the ore bauxite) to aluminum:

                   \(2 \mathrm{Al}_{2} \mathrm{O}_{3}(s) \longrightarrow 4 \mathrm{Al}(s)+3 \mathrm{O}_{2}(g) \quad \Delta H=+3350 \mathrm{~kJ} / \mathrm{mol}\)

(a) Is the reaction exothermic or endothermic?

(b) How many kilojoules are required to produce 1.00 mol of aluminum?

(c) How many kilojoules are required to produce 10.0 g of aluminum?

Text Transcription:

2 Al_2 O_3(s) longrightarrow 4 Al(s)+3 O_2(g) quad Delta H=+3350/kJ mol

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