The question is: What is the molarity of the copper (II) chloride solution your teacher provided? Show calculations. Obtain the true molarity of the copper (II) chloride solution and calculate percent error.
I have done this so far trying to answer the question:
Molar Mass: (26.98) (134.45) (63.55) (133.33)
Balanced eq: 2Al + 3CuCl2 ---> 3Cu + 2AlCl3
Mol-Mol ratio: 2 3 3 2
# of moles: 0.032 0.048 0.048 0.032
Amount: 0.86g 6.45g 3.05g 4.26g
^ (0.86g is the average mass of Al
used in the lab.)
To find percent error my teacher gave me the formula:
% Error=Value experimental-Value accepted
____________________________x100
Value accepted
My teacher also said that 0.25 M is the accepted and 0.6g is the experimental.
In this lab we put an aluminum strip into a copper(II) chloride solution to see which was the limiting reactant. I need help answering the question I wrote above. Thanks!
2 answers