What Happens When Aluminium Reacts with Chlorine in Water?

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Discussion Overview

The discussion revolves around the chemical reaction between aluminium and chlorine in water, focusing on the reaction's thermodynamics, the calculation of moles, and the state of water after the reaction. Participants explore the concepts of balancing chemical equations, limiting reagents, and heat transfer in the context of a homework problem.

Discussion Character

  • Homework-related, Technical explanation, Mathematical reasoning

Main Points Raised

  • One participant requests an explanation of the reaction, asking whether it is endothermic or exothermic and how colligative properties relate to the question.
  • Another participant attempts to balance the chemical equation for the reaction and calculates the moles of aluminium and chlorine, expressing uncertainty about the accuracy of their work.
  • A participant questions whether finding the change in temperature is necessary to determine the state of water after the reaction.
  • There is a reiteration of the balanced equation, with a note that chlorine is diatomic, and a suggestion to find the limiting reagent to calculate the moles of AlCl3 produced and the heat generated.
  • One participant acknowledges a potential mistake in their calculations and expresses intent to re-evaluate their approach based on feedback.

Areas of Agreement / Disagreement

Participants do not reach a consensus on the balancing of the chemical equation or the calculations involved. There is ongoing uncertainty regarding the correct approach to the problem.

Contextual Notes

Participants express limitations in their understanding of the reaction and calculations, particularly regarding the treatment of chlorine as diatomic and the implications for stoichiometry and thermodynamics.

ShakeSpee
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Hi, thanks for checking out this thread.

I'm really having a problem with the question because I don't have any foundation.

If you could, would you:
Explain what exactly is going on? Is this an endothermic or exothermic reaction?
What are colligative properties, and what do they have to do with this question?

Homework Statement



10.0 g Aluminium and 21.0 g Chlorine react in a solution of water. Ignoring colligative properties, what will the state of water be if 1000.0g starts at 10.0°C and a heat of formation of 92kJ/mol of product?

Thanks again for taking the time to help.
--ShakeSpee
 
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Okay, so far I think I balanced the equation (but I don't think I did it correctly.)
1 Al(s) + 3 Cl(l) -----> 1AlCl3 +H20 + energy

I also calculate the amount of moles. (.371 mol Al, 1.777 mol Cl)

Is this correct?
 
Now I'm stuck; do I have to find the change in temperature to find the state of water?
 
ShakeSpee said:
Okay, so far I think I balanced the equation (but I don't think I did it correctly.)
1 Al(s) + 3 Cl(l) -----> 1AlCl3 +H20 + energy

Chlorine is diatomic (not that it will change the result in this case).

I also calculate the amount of moles. (.371 mol Al, 1.777 mol Cl)

Al is OK, Cl is not (regardless of whether it is to be treated as atomic, or diatomic).

You need to find the limiting reagent and calculate number of moles of AlCl3 produced. Then you will be able to calculate amount of heat produced, and use it to calculate new water temperature.
 
Borek said:
Chlorine is diatomic (not that it will change the result in this case).
Al is OK, Cl is not (regardless of whether it is to be treated as atomic, or diatomic).

You need to find the limiting reagent and calculate number of moles of AlCl3 produced. Then you will be able to calculate amount of heat produced, and use it to calculate new water temperature.
I thought that was where my mistake was! I try it again, thanks!
 

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