Solid aluminum Al and chlorine Cl2 gas react to form solid aluminum chloride AlCl3 . Suppose you have 5.0 mol of Al and 2.0 mol of Cl2 in a reactor. Suppose as much as possible of the Al reacts. How much will be left? Round your answer to the nearest 0.1 mol .
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
Solid aluminum
and chlorine
gas react to form solid aluminum chloride
. Suppose you have
of
and
of
in a reactor.
Suppose as much as possible of the
reacts. How much will be left? Round your answer to the nearest
.
Aluminium and chlorine react to form aluminium chloride. The equation form the balanced chemical reaction is as follows:
The moles of Al is = 5.0 mole
The mole of chlorine is = 2.0 mole
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
![**Chemical Reaction of Aluminum and Chlorine**
---
Solid aluminum (Al) and chlorine (Cl₂) gas react to form solid aluminum chloride (AlCl₃). Suppose you have 2.0 mol of Al and 1.0 mol of Cl₂ in a reactor.
**Problem Statement:**
What would be the limiting reactant? Enter its chemical formula below.
---
Explanation:
- **Reactants:**
- Aluminum (Al) - 2.0 mol
- Chlorine (Cl₂) - 1.0 mol
- **Product:**
- Aluminum Chloride (AlCl₃)
To solve this, you will need to use the stoichiometry of the balanced chemical equation:
\[ 2Al + 3Cl₂ \rightarrow 2AlCl₃ \]
From the equation, you can see that 2 moles of aluminum react with 3 moles of chlorine gas to form 2 moles of aluminum chloride. By comparing the mole ratio of the reactants you have to the ratio in the balanced equation, you can determine which reactant will be consumed first, thereby identifying the limiting reactant.
Given that only 1.0 mole of Cl₂ is available and the reaction requires 3 moles of Cl₂ for every 2 moles of Al:
Calculate:
- Moles of Cl₂ required for 2 moles of Al: \( (2 \text{ moles Al}) \times \left(\frac{3 \text{ moles Cl₂}}{2 \text{ moles Al}}\right) = 3 \text{ moles Cl₂} \)
Since only 1.0 mole of Cl₂ is available (which is less than the required 3 moles), Cl₂ is the limiting reactant.
---
**Interaction with the Diagram:**
The diagram appears to have an input box accompanied by options for submission, which might include typical operations like 'Check Answer', 'Reset', and 'Help'. The chemical formula of the limiting reactant (in this case, Cl₂) should be input into the input box provided in the diagram for validation.
---](https://content.bartleby.com/qna-images/question/cc60b291-b343-46d1-985f-51e0feae8cbd/2a61dea8-d995-49ca-b757-b7894f52bf49/w8h4u2_processed.png)
by Bartleby Expert
