Lab of moles of iron and copper

Topics: Chemistry, Atom, Molecule Pages: 3 (440 words) Published: February 5, 2014
Moles of Iron and Copper Lab

Data and Observations
Before the reaction:
Mass of empty, dry beaker: 153.44g
Mass of beaker + copper (II) chloride: 161.44g
Mass of two iron nails: 7.27g
After the reaction:
Mass of two iron nails: 6.29g
Mass of beaker + copper (dry): 154.50g

Questions and Calculations
1. a) Mass of two iron nails before the reaction
– Mass off two iron nails after the reaction
= Mass of iron used in the reaction
= 7.27g – 6.29g
= 0.98g of iron used in the reaction

b) Mass of beaker + copper (II) chloride
– Mass of empty, dry beaker
= Mass of copper (II) chloride used
= 161.44g - 153.44g
= 8g of copper (II) chloride used

c) Mass of beaker + copper (II) chloride
– Mass of beaker + copper (dry)
= Mass of copper produced
= 161.44g – 154.50g
= 1.06g of copper produced

2. a) 0.98g x 1 mol = 0.018 moles of iron used

b) 1.06g x 1 mol = 0.0167 moles of copper produced

3. a) 1.8 x 10-2 moles x 6.02x1023molecule x 1 atom = 1.1 x 1022 atoms of iron used 1 mol 1 molecule

b) 1.67 x 10-2 moles x 6.02x1023 molecule x 1 atom = 1.01 x 1022 atoms of copper produced 1 mol 1 molecule

4. The ratio of moles of copper produced to moles of iron used Fe = 0.018/0.018 = 1 Cu = 0.018 /0.0167 = 1.08
Fe:Cu = 1:1.08
This is inaccurate as it should have been 1:1 ratio of moles of copper produced to moles of iron used because the law of conservation of mass states that the mass of substances produced by a chemical reaction is always equal to the mass of reacting substances. But in my opinion, I think I did a good job of making it even without even noticing! It was a close call.

5. There is a possibility that there was some of the copper (II) chloride left in the beaker due...
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