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.
yes
This is a 'Sngle Displacement' reaction ( A + BC --> AC + B
Silver (Ag)
The reduction potential plus oxidation potential is negative.
Cr(s) | Cr3+(aq) Pb2+(aq) | Pb(s)
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).
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.
yes
I cannot answer this question.
In the reaction ( 2Ag^{+} + 2e^{-} \rightarrow 2Ag ), two electrons are transferred per silver ion, so a total of four electrons are transferred in the overall reaction.
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.
No, balancing the equation is not necessary to determine if a redox reaction is occurring. In this case, the species involved are chromium ions, so the hydrogen ions are just spectators. The reaction would be identified as non-redox because the oxidation states of chromium do not change.
This is a 'Sngle Displacement' reaction ( A + BC --> AC + B
Silver (Ag)
The standard reduction potentials for Mg/Mg^2+ and Cu^2+/Cu are -2.37 V and +0.34 V, respectively. To determine the overall cell potential, you subtract the reduction potential of the anode (Mg/Mg^2+) from the reduction potential of the cathode (Cu^2+/Cu) since the anode is where oxidation occurs. Therefore, the overall cell potential would be 0.34 V - (-2.37 V) = 2.71 V.
yes as zinc is oxidised and hydrogen is reduced
In the redox reaction, silver (Ag) has been reduced because it gains electrons in forming solid silver (Ag) from silver nitrate (AgNO3).