2Cu + O2 -> 2CuO
Now you have an ionic bond because the oxygen has taken two electrons from copper into it's valance shell. Thus, copper is oxidized; loses electrons.
Zinc (Zn) can be oxidized more easily compared to copper (Cu) because zinc has a lower standard reduction potential. This means that zinc is more likely to lose electrons and be oxidized in a redox reaction.
In this reaction, zinc (Zn) is oxidized to form zinc sulfate (ZnSO4) while copper (Cu2+) in copper sulfate (CuSO4) is reduced to copper (Cu). The zinc loses electrons (oxidized) to form zinc sulfate, while the copper gains electrons (reduced) to form solid copper.
no reaction because Cu is below Zn at electrochemical series ,so Cu can't take Zn away from its salts
Since oxygen is diatomic it requires 2 moles of oxygen.
To find the amount of copper oxide produced, we need to determine the limiting reactant. The balanced equation is 4Cu + O2 → 2Cu2O. Calculate the moles of each reactant: 127g Cu / 63.5 g/mol Cu = 2 moles Cu, and 32g O2 / 32 g/mol O2 = 1 mole O2. Since 1 mole of O2 is needed for 4 moles of Cu, O2 is the limiting reactant. Hence, 2 moles Cu will react with 1 mole O2 to produce 2 moles Cu2O, which is 63.5 x 2 x 2 = 254g Cu2O.
Cu is oxidized. The oxidation number goes from 0 in Cu to +2 in CuSO4. S is reduced. The oxidation number goes from +6 in H2SO4 to +4 in SO2. The oxidizing agent is H2SO4 since it causes Cu to be oxidized. The reducing agent is Cu since it causes S in H2SO4 to be reduced.
Zinc (Zn) can be oxidized more easily compared to copper (Cu) because zinc has a lower standard reduction potential. This means that zinc is more likely to lose electrons and be oxidized in a redox reaction.
In this reaction, zinc (Zn) is oxidized to form zinc sulfate (ZnSO4) while copper (Cu2+) in copper sulfate (CuSO4) is reduced to copper (Cu). The zinc loses electrons (oxidized) to form zinc sulfate, while the copper gains electrons (reduced) to form solid copper.
The final answer would be 2Cu O2---> 2CuO
The chemical reactions are:4 Cu(I) + O2 = 2 Cu2O2 Cu(II) + O2 = 2 CuO
Cu(s)
oxidized
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cupper (II) oxide
oxygen
Iron (Fe) is a metal that can be oxidized by two common ions: copper ions (Cu^2+) and silver ions (Ag^+).
Copper has 2 possible valence configurations: Cu+1 or Cu+2. In either case, the products would be Copper oxide but their chemical characteristics, and their formulas, would be different, due to the difference in valence.For Cu+1, the product would be a red powder, of the formula, Cu2O.For Cu+2, the product would be a black powder, of the formula, CuO