Did I Calculate the Moles and Mass Correctly in My Iron and Copper Lab?

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    Copper Iron Lab Moles
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Discussion Overview

The discussion revolves around the calculations of moles and mass in a chemistry lab involving the reaction between iron and copper chloride. Participants are seeking verification of their results and assistance with specific questions related to their experimental data.

Discussion Character

  • Homework-related
  • Mathematical reasoning
  • Debate/contested

Main Points Raised

  • One participant presents their experimental data and calculations for the mass and moles of copper and iron, expressing uncertainty about the accuracy of their results.
  • Another participant suggests that the calculation for the mass of copper is based on the difference between the weight of copper chloride and the formed copper, indicating a misunderstanding of the question asked.
  • A later post corrects the mass of the beaker, which affects the calculations, leading to a revised mass of copper formed.
  • Participants discuss the mole ratio, with one expressing doubt that it could be 1:1 or 2:3, suggesting that something is wrong with their calculations.
  • There is a request for further assistance in answering the initial questions posed by the original poster.

Areas of Agreement / Disagreement

Participants express differing views on the calculations, with some agreeing on the need for corrections while others remain uncertain about the mole ratio and the accuracy of the mass measurements. The discussion does not reach a consensus on the correct values or methods.

Contextual Notes

Limitations include potential errors in mass measurements and calculations, as well as misunderstandings regarding the definitions of substances involved in the reaction.

Who May Find This Useful

Students and educators involved in chemistry labs, particularly those focusing on stoichiometry and reaction calculations.

JenniferBlanco
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Can someone please verify my results? and help me in one-2 questions?

I did this lab in school today and had some problems filling in the table that followed.
In the lab, we took some Copper Chloride and mixed it dionized water. Then we added in an iron nail and waited for about 20 mins. After 20 mins we decanted the water(threw it away) and were left with copper+a lil bit of water which was later dried.
The following is the data I have

Mass of Beaker --> 0.906
Mass of Beaker and Copper Chloride --> 12.44
Mass of Nail before reaction-->1.729
Mass of Nail after reaction-->1.444
Mass of Beaker and dry copper[dry]-->10.345

The questions that followed were to calculate moles and mass.

1>Mass of Copper formed.

For this,it should be 12.44-10.345 =2.095gms

2>Moles of Copper

For this I did 2.095/63.5= .329moles

3>Mass of Iron reacted
1.729-1.444=.285gms4>Moles of Iron
.285/55.8=.005

5>Ratio of moles of Iron to Copper
_______________________________________________

I guess I screwed up on the calculations or something on the Mass of Iron Reacted which gave me .285 gms. This I feel has screwed my moles of Iron up. I don't know where I am going wrong in this.

If someone can help me out,I would be greatful. I am kinda guessing the mole ration should be 1:1.Jen
 
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Can Anyone atleast get me started? :cry:
 
?Anyone?
 
Everything looks good, except that your calculation for mass of copper is actually the difference in the weight of copper chloride and formed copper. The answer is correct but that question was not asked.

All of your problems are solved if you can find a weigh to determine the mass of copper.

Copper chloride is not copper.
 
I messed up on the Mass of the beaker. it should read 9.906 above and not .906

In the end when we dried the copper from the dionized water,I massed it and got 10.345gms for copper.

The mole ration after calculation is a high number and not 1:1 or 2:3. I am sure something is wrong.
 
Last edited:
Answer the first question!
 
First Question?

So copper should be =10.345-9.906-->.439gms
 
Excellent!

Couple that answer with your obvious skill in problem-solving and you are done with this problem!

Now answer #2 and recalculate #5.
 

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