Asked by Rosio
A considerable amount of heat is required for the decomposition of aluminum oxide shown below. What is the heat change when 3.5 moles of aluminum oxide are decomposed? Is this endothermic or exothermic?
2Al2O3(s) → 4Al(s) + 3O2(g) ΔH = 3352kJ
2Al2O3(s) → 4Al(s) + 3O2(g) ΔH = 3352kJ
Answers
Answered by
DrBob222
2Al2O3(s) → 4Al(s) + 3O2(g) ΔH = 3352kJ
If the reaction shown is 3352 kJ FOR THE REACTION AS SHOWN, then
dH for the question = 3352 kJ x (3.5/2) = ?
If dH is + this is an endothermic reaction.
If the reaction shown is 3352 kJ FOR THE REACTION AS SHOWN, then
dH for the question = 3352 kJ x (3.5/2) = ?
If dH is + this is an endothermic reaction.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.