yes
This is a 'Sngle Displacement' reaction ( A + BC --> AC + B
Silver (Ag)
The reduction potential plus oxidation potential is negative.
The overall redox reaction of Cr2O7 + Br is not a balanced equation. To balance the equation, the half-reactions for the oxidation and reduction of each element need to be determined and balanced first.
Cr(s) | Cr3+(aq) Pb2+(aq) | Pb(s)
4Li + O2 -> 2Li2O
This is a 'Sngle Displacement' reaction ( A + BC --> AC + B
No, it is not a redox reaction. None of the oxidation numbers changes during the reaction. You have to determine the oxidation number for each element and see if it changes from reactant side to product side. If the oxidation number doesn't change, it is not a redox reaction.
Sodium (Na) has been reduced.
yes as zinc is oxidised and hydrogen is reduced
Yes, the reaction between Zn and CuCl2 to form ZnCl2 and Cu is a redox reaction. Zinc (Zn) is oxidized to form Zn2+ ions, while copper (Cu2+) is reduced to elemental copper (Cu).
I cannot answer this question.
The redox reaction you provided is unbalanced. The correct balanced redox reaction should be 2Cl + Br2 -> 2Cl- + 2Br. This balanced equation ensures that both charge and mass are conserved during the reaction.
Silver (Ag)
In the redox reaction, silver (Ag) has been reduced because it gains electrons in forming solid silver (Ag) from silver nitrate (AgNO3).
In the redox reaction AgNO3 + NaNO3 + Ag, silver (Ag) is reduced from Ag+ to Ag with the gain of one electron. Therefore, one electron is transferred in this reaction.
Yes, this is a redox reaction because there is a transfer of electrons between the reactants (Al losing electrons to become AlCl3, which is reduced, and H+ ions gaining electrons to become H2 gas, which is oxidized).