here is the remaining part of my lab report , i need help filling it up Molar ma

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here is the remaining part of my lab report , i need help filling it up

Molar mass of Cu^. Theoretical yield of copper metal in grams (mass of Cd^expected to be formed) Percent yield of copper metal (includes accuracy) What experimental errors occurred during your experiment that may have caused something other than 100% yield of copper metal? Use complete sentences and cite more than one example. Aluminum Using the stoichiometry given in Eq. 1 and the mass of copper recovered (see data section), predict the theoretical mass of aluminum that reacted. Compare the amount of aluminum you predict has reacted with the amount you determined experimentally (see data section of report) using the percent error equation (See Appendix B) In complete sentences summarize observations during the experiment, including any changes to the solution and aluminum wire as a result of the reaction? Mass of copper(II) chloride CuCl_2 _____ Mass of aluminum _____ Mass of aluminum remaining after reaction. ______ Mass of aluminum that reacted. ______ Mass of filter paper and watchglass._____ Mass of filter paper, watchglass, and copper._____ Mass of copper recovered._____ Show calculations with each blank except for the molar mass of Cu^(Unless otherwise noted, for blanks including calculations in this section) Copper Molar mass of Cucl_2 Mole of CuCl_2 dissolved Balanced equation for the dissociation of CuCl_2 in water Mole of copper(II) ions (Cu^2+) initially in solution Balanced net ionic equation for the reaction of copper (II) chloride with aluminum Mole of copper metal (Cu^0) expected to be formed.

Explanation / Answer

ANS:

Thus , no. Of moles= mass/ molar mass

So, moles of Cu2+ ions = 3.051 g/ 134.45 = 0.0226 moles

2. Moles of copper metal expected to be formed:

Mass of Cu recovered= 1.307 g

Molar mass of Cu = 63.55 g

Therefore, moles of Cu expected to be formed= 1.307/63.55

= 0.0205 moles

3. Molar mass of Cu0 = 63.55 g/mol

4. Theoretical yield of Cu metal:

Moles of CuCl2/coefficient of CuCl2 =moles of Cu/coefficient

And no. Of moles = given mass/ molar mass

Therefore,

(Mass of CuCl2/molar mass of CuCl2)/ coefficient =

( Mass of Cu/molar mass of Cu)/ coefficient

Putting up all the values ,

Mass of Cu(theoretical) = 3.051 ×3 ×63.55 / (134.55 ×3)

   = 1.4421 g

5. percent yield:

Percent yield = (actual yield/ theoretical yield)×100

= (1.3070/ 1.4421)× 100 = 90.63%

Aluminium:

1. Theoretical mass of Al that reacted: As per the chemical reaction, 3 moles of CuCl2 react with 2 moles of Al.

So, 0.0226 moles of CuCl2 will react with = 0.0226 × 2/3 =0.0150 moles

Thus, theoretical mass of Al that reacted= moles × molar mass = 0.0150 mole× 27.00 g/mole = 0.4050 g

2. Percent error:

Expected mass of Al that reacted= 0.425 g

Thus percent error= (0.424-0.4050)/ 0.4050

   =0.049%

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