Consider the following reaction:
2Al(s)+ 3Cl₂(g) $\to$ 2AlCl₃(s); $\Delta$ H = -1390.81 kJ
a)Is the reaction exothermic or endothermic?
b)How much heat is produced/required when 10.0 g AlCl₃ forms.
c)How many grams of Al are required to absorb/evolve 1.00 kJ of energy?

Question

Consider the following reaction:
2Al(s)+ 3Cl₂(g)

\to

2AlCl₃(s);

\Delta

H = -1390.81 kJ
a)Is the reaction exothermic or endothermic?
b)How much heat is produced/required when 10.0 g AlCl₃ forms.
c)How many grams of Al are required to absorb/evolve 1.00 kJ of energy?

Quizplus · Accepted Answer

The Answer of Consider the following reaction: 2Al(s)+ 3Cl₂(g)$\to$2AlCl₃(s);$\Delta$H = -1390.81 kJ a)Is the reaction exothermic or endothermic? b)How much heat is produced/required when 10.0 g AlCl₃ forms. c)How many grams of Al are required to absorb/evolve 1.00 kJ of energy?

Consider the Following Reaction: 2Al(s)+ 3Cl2(g) →\to→ 2AlCl3(s); Δ\DeltaΔ H = -139081 KJ A)Is the Reaction Exothermic or Endothermic? B)How Much

Consider the Following Reaction:
2Al(s)+ 3Cl₂(g) $\to$ 2AlCl₃(s); $\Delta$ H = -139081 KJ
A)Is the Reaction Exothermic or Endothermic?
B)How Much