Joel reacted 0.9845 g of iron filings with an excess of copper sulphate solution. When the reaction was complete the solution had changed from blue to green and a copper deposit weighing 1.024 g had formed in the solution. In this reaction, metallic iron is converted into ferrous ion (Fe2+) and cupric ion (Cu2+) is converted into metallic copper.

a) Calculate the number of moles of iron used and the number of moles of copper

formed.

b) Calculate the theoretical mass of copper that was expected to be produced and

hence deter,mine the percentage yield of Joel’s experiment.

c) How many molecules of iron are present in 0.9845 g of iron fillings?

Fiona prepared a solution by dissolving 1.35 g of silver nitrate in a 250 mL volumetric flask and diluting it up to the volume.

d) Calculate the molarity of the silver nitrate solution.

e) What volume of this solution is required to prepare 100 mL of 0.01 M of silver nitrate solution?

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pstnonsonjoku pstnonsonjoku · Answer 1 · 2022-05-02T14:41:33+02:00

From the stoichiometry of the reaction, the percentage yiled of the copper is 89.6%

The reaction equation here is given as; Fe(s) + CuSO4 (aq) ----->FeSO4(aq) + Cu(s)

Number of moles of Fe = 0.9845 g/56 g/mol = 0.018 moles. Since the reaction is 1:1, this is also the number of moles of Cu formed.

Theoretical yiled of Cu = 0.018 moles * 63.5 g/mol = 1.143 g

Percentage yiled = 1.024 g/1.143 g * 100/1 = 89.6%

If 1 mole of Fe contains 6.02 * 10^23 molecules

0.018 moles of Fe contains 0.018 moles * 6.02 * 10^23 molecules/1 mole = 1.1 * 10^22 molecules.

Number of moles of AgNO3 = 1.35 g/170 g/mol = 0.0079 moles

Molarity of the solution = 0.0079 moles/250 * 10^-3 L = 0.0032 M

Hence; 0.0032 M * V1 = 100 mL * 0.01 M

V1 = 312.5 mL

Learn more about stoichiometry: https://brainly.com/question/9743981

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