Objective: To observe the single replacement reaction between iron and copper(II) sulfate,
calculate the mole ratio and find percent error.
Theory:
Mole relations: One mole (abbreviated mol) is equal to 6.02×10 23 molecular entities (Avogadro's number). Each element has a different molar mass depending on the weight of 6.02×10 23 of its atoms (1 mole). The total number of atoms of each element must be the same on each side of the equation to satisfy the Law of Conservation of Mass. The experiment aides in the understanding of mole-mass relationships that exist in a chemical reaction and in the interpretation of a balanced chemical equation.
Oxidation and reduction: Oxidation is the loss of electrons or an increase in oxidation state by a
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molecule, atom, or ion. Reduction is the gain of electrons or a decrease in oxidation state by a molecule, atom, or ion. Materials: 100 mL beaker, any size beaker, stir rod, wash bottle, 50 mL graduated cylinder, weigh paper, electronic balance, goggles, hot plate scoopula, hot mitts, CuSO4, iron fillings. Procedure (Day 1): A 100mL beaker was labelled with students’ names. The 100 mL beaker was weighed and it’s mass recorded. 10g of CuSO4 was added to the 100mL beaker. 30 mL of distilled water was added to the CuSO4. The solution was heated on a hotplate until it started to boil (tongs were used to remove the beaker from the hotplate). A sheet of weigh paper was placed on the balance and 2g of iron fillings were shaken out and massed to 2 decimal places. Whilst stirring slowly, small amounts of iron fillings were shaken into the hot CuSO4 solution. The CuSO4 solution was left to sit for 10 minutes. The solution was carefully poured into the second beaker without losing any of the solid. 10 mL of distilled water was added to the solid residue and stirred. Then the solution was poured into the other beaker. This washing was repeated three times. The beaker with solid inside was placed in the fume hood to dry overnight. Procedure (Day 2): 11. The mass of the dry beaker and the copper residue was determined and recorded. Results and Calculations: Qualitative Results: The copper (II) sulfate was a light blue, chunky, opaque, dull powder. The copper (II) sulfate solution was blue and transparent. The iron powder was black and opaque. The copper produced was a red and black clumpy opaque powder.
Quantitative Results:
Mass of empty beaker and label
50.95g
Mass of iron fillings
2.00g
Mass of beaker and dry copper
53.23g
Molar mass of copper
63.55g
Calculations:
Number of moles of iron used: nFe = m = 2.00g Fe =0.03581 = 3.58 x 10-2 mol
M 55.85g/mol
Mass of copper produced: mCu= 53.23 - 50.95= 2.28 g
Number of moles of copper produced: nCu= m = 2.28 = 0.0358=3.58x10-2 mol
M 63.55
Unreduced ratio mol of iron used : 3.58 x 10-2 mol Fe : 3.58 x 10-2 mol Cu
mol of copper produced
Simplified mol ratio: 1 mol Fe :1 mol Cu
Percent Error: %Error= I actual - theoretical I x 100 = l2.28 - 2.28l x 100 = 0 %
Theoretical
2.28 Conclusion: The total mole ratio was 1:1 and the percent error was 0% Error Analysis: Although there was none, various sources of error could have played a part in this experiment, including: incomplete washing, incomplete chemical reaction, procedural techniques, and any foreign material still present in the beaker at the time of the final weighing. Because the percent error was equal to zero, the accuracy of each measurement must have been absolute.
11.) Subtract the mass of the evaporating dish from the mass of the evaporating dish and it's contents. Multiply that number by 10 to get the solubilty in grams per 100 cm3 of water.
When the flame was blown out and the glowing wooden splint was placed halfway into the test tube containing H2O2 and MnO2 crystals, the splint reignited and caught flame once again. This demonstrates the decomposition of H2O2 into water and hydrogen. MnO2 is a catalyst that increases the rate at which H2O2 decomposes. Adding oxygen to a fire will cause it to burn faster and hotter and the oxygen rich test tube allowed the splint to reignite.
Cu (aq) + 2NO3 (aq) + 2Na+ (aq) + 2OH- (aq) → Cu(OH)2 (s) + 2Na+ (aq) + 2NO3(aq)
Discussion: The percent of errors is 59.62%. Several errors could have happened during the experiment. Weak techniques may occur.
Measure the weight of a small stone to fit inside the opening of a 50ml graduated cylinder.
5) Find the experimental mass of both the c-clamp and the empty pan by using the formula from page one. Record this as mtotal.
Remove the extra solvent on a steam bath under a hood while flushing the flask with N2 gas, leaving the crude extract. Weigh extract.
After the calculation we needed to convert pc to meters so we used the calculation factor of 1pc=3*10^16m
The beginnings of modern processing of iron can be traced back to central Europe in the mid-14th century BC. Pure iron has limited use in today’s world. Commercial iron always contains small amounts of carbon and other impurities that change its physical properties, which are much improved by the further addition of carbon and other alloying elements. This helps to prevent oxidation, also known as rust.
When it is finished heating, close the Bunsen burner and leave the crucible to cool down. 8. Measure and weight the content and the crucible. Table Mass of crucible (g) Mass of crucible and baking soda(g)
get it exactly correct or you may not be able to measure the amount of
[6] Hayrynen KathyL., (2002) The Production of Austempered Ductile Iron (ADI), World Conference on ADI.
It was necessary to calculate the surface area of the aggregate to find out if adjustments needed to be made to the amount of binder that was required a simple formula was used to provide this information (Shell Bitumen 1991): T= b/(100-b) x 1/Db x 1/SAF