How many atoms of copper reacted? How many atoms of copper reacted? In this reac
ID: 490809 • Letter: H
Question
How many atoms of copper reacted? How many atoms of copper reacted? In this reaction, for each mole of solid copper that reacts, one mole or copper (II) nitrate were produced in your reaction beaker? Rxn 2 - copper(II) nitrate with sodium hydroxide: In this reaction, for each mole of copper(II) nitrate that reacts, one mole of copper(lI) hydroxide is produced. How many moles of copper(II) nitrate were produced in your reaction beaker? How many moles of nitrate ion were produced? Rxn 3 - copper(II) hydroxide heated to become copper(II) oxide: What is the molecular mass of copper(II) hydroxide? What is the molecular mass of copper(II) oxide? In this reaction, for each mole of copper(ll) hydroxide that reacts, one mole of copper(II) oxide is produced. How many moles of copper(II) oxide were produced in your reaction beaker? If you could recover the copper(II) oxide from the solution and measure its mass, what would its mass in grams be? Rxn 4 - copper(II) oxide with hydrochloric acid: How many moles of hydrochloric acid were required to completely react the copper(II) oxide in your beaker? In this reaction, for each mole of copper(II) oxide that reacts, one mole of copper(II) chloride is produced. How many moles of copper(II) chloride were produced in your reaction beaker? Rxn 5 - copper(II) chloride with aluminum: How many moles of aluminum were added? How many atoms of aluminum were added? In this reaction, for each mole of copper(II) chloride that reacted, one mole of solid copper is produced. How many moles of copper should be recovered from your beaker? How many moles of copper were actually recovered and what is the mass percent recovery of the copper?Explanation / Answer
Ans. Reaction 1. Cu(s) + HNO3 -----------> Cu(NO3)2
#1. Moles of Cu reacted = Mass / Formula mass = 0.9 g / (63.546 g/mol) = 0.001685 mol
#2. Atoms Cu reacted = Moles x Avogadro number
= 0.001685 mol x (6.022 x 1023 atom/ mol)
= 0.014 mol
#3. Moles of Cu(II) nitrate formed = Mass of Cu(II)nitrate produced / its molar mass
= 146.4 g/(187.55588 g/ mol)
= 0.780 mol
Note: moles of Cu(NO3)2 can’t be greater than moles of Cu(s) because 1 mol Cu produces 1 mol Cu(II) nitrate.
So, kindly recheck your values.
The further calculations are being made for explanation only, kindly put correct experimental values while you make calculation.
Reaction 2. Cu(NO3)2 + 2NaOH -----> Cu(OH)2 + 2NaNO3
#4. Moles of Cu(II) nitrate produced in beaker = 0.78 mol ; (from #3.)
#5. Note stoichiometry: 1 mol Cu(NO3)2 produces 2 mol nitrate ion.
So, moles of nitrate ion = 2 x mole of Cu(NO3)2
= 2 x 0.78 mol = 1.56 mol
Reaction 3.
#6. Molar mass of Cu(OH)2= 97.56 g/mol
#7. Molar mass of CuO = 79.54 g/mol
#8. Moles of CuO = moles of Cu(OH2) = moles of Cu(NO3)2 produced
= 0.78 mol ; [see stoichiometry of reaction 2]
#9. Mass of CuO recovered (theoretical yield) = Moles of CuO x Molar mass
= 0.78 mol x (79.54 g/mol)
= 62.04 g
Reaction 4: CuO + 2 HCl = CuCl2 + H2O
#10. Stoichiometry: 1 mol CuO requires 2 mol HCL for complete reaction.
So, moles of HCl required = 2 x moles of CuO
= 2 x 0.78 mol = 1.56 mol
#11. Stoichiometry: 1 mol CuO requires produces 1 mol CuCl2.
So, moles of CuCl2 produced =- moles of CuO = 0.78 mol
Reaction .5.
#12. Moles of Al added = Mass/ Atomic mass
= 0.92 g/ (26.98 g/mol) = 0.034 mol
#13. Atoms of Al = 0.034 mol x (6.022 x 1023 atom/ mol) = 2.05 x 1022 atoms
#14. Moles of Cu recovered = Moles of CuCl2 reacted = 0.78 mol
#14. Initial mole of Cu = 0.014 mol ; [see #2.]
Note: As mentioned in Notes, #3, there is error with recovered Cu(II)nitrate in the beaker. Please put correct experimental values to get correct outcomes.
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