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What is the standard reduction potential E for the halfreaction Al3 plus aq plus 3e?
-1.68 V
What is the standard reduction potential for the half reaction Zn2 plus plus 2e- equals Zn?
Zn2+ + 2e- <--> Zno -0.7618 V
What is the standard reduction potential E for the half reaction mf2 plus plus 2e - mg?
The standard reduction potential (E°) for the half-reaction ( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg} ) is approximately -2.37 V. This indicates that magnesium ions are reduced to magnesium metal, but the reaction is not favorable under standard conditions due to its negative potential. The value reflects magnesium's strong tendency to lose electrons and form cations, characteristic of its placement in the reactivity series of metals.
How can one determine if a redox reaction will be non-spontaneous?
The reduction potential plus oxidation potential is negative.
The reaction CuO plus CO yields Co2 plus Cu is an example of oxidation or reduction or both or neither?
The reaction CuO + CO → CO2 + Cu is an example of reduction because copper(II) oxide (CuO) gains electrons to form copper (Cu). Reduction is the gain of electrons by a species.
What is the standard reduction potential E for the halfreaction Al3 plus aq plus 3e?
-1.68 V
What is the standard reduction potential for the half reaction Zn2 plus plus 2e- equals Zn?
Zn2+ + 2e- <--> Zno -0.7618 V
What is the standard reduction potential E for the half reaction mf2 plus plus 2e - mg?
The standard reduction potential (E°) for the half-reaction ( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg} ) is approximately -2.37 V. This indicates that magnesium ions are reduced to magnesium metal, but the reaction is not favorable under standard conditions due to its negative potential. The value reflects magnesium's strong tendency to lose electrons and form cations, characteristic of its placement in the reactivity series of metals.
How can one determine if a redox reaction will be non-spontaneous?
The reduction potential plus oxidation potential is negative.
What is the overall voltage for a redox reaction with the half reactions Mg s -- Mg2 plus plus 2e- and Cu2 plus -- Cu s?
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.
If silver and copper are used to make a cell what half-reactions will occur for ag plus aq plus e- ag s e0 equals 0.80 v and for cu2 plus aq plus 2e- cu aq e0 equals 0.34 V?
In the cell, the half-reaction for silver will be Ag+ (aq) + e- -> Ag (s) with a standard reduction potential of +0.80 V. The half-reaction for copper will be Cu2+ (aq) + 2e- -> Cu (s) with a standard reduction potential of +0.34 V. The silver half-reaction will occur at the cathode, while the copper half-reaction will occur at the anode in the cell.
WHAT IS THE OVERALL VOLTAGE FOR A REDOX REACTION HE HALF REACTIONS AG plus E-ag(S) AND CU(S) CU2 plus 2E?
To determine the overall voltage for the redox reaction involving the half-reactions ( \text{Ag}^+ + e^- \rightarrow \text{Ag}(s) ) and ( \text{Cu}(s) \rightarrow \text{Cu}^{2+} + 2e^- ), we first need the standard reduction potentials. The standard reduction potential for silver (( \text{Ag}^+ )) is +0.80 V, and for copper (( \text{Cu}^{2+} )) is +0.34 V. Since silver is reduced and copper is oxidized, the overall cell potential is calculated as ( E_{\text{cell}} = E_{\text{reduction}} - E_{\text{oxidation}} = 0.80 , \text{V} - 0.34 , \text{V} = 0.46 , \text{V} ). Thus, the overall voltage for the redox reaction is +0.46 V.
Is TiCl3 plus Mg equals Ti plus MgCl2 an oxidation reduction?
Absallutly!
3000 plus 50 plus 0.009 in standard notation?
3000 plus 50 plus 0.009 in standard notation is 3,050.009
What is 2000000000 plus 70000000 plus 100000 plus 70000 plus 3000 plus 800 plus 10 in standard form?
In standard form:2,000,000,00070,000,000100,00070,0003,000800+ 10________________2,070,103,810
Can Sn reduce Zn with 2 plus oxidation number under standard- state conditions and why?
No, tin (Sn) cannot reduce zinc (Zn) with a +2 oxidation number under standard-state conditions. This is because the standard reduction potential of Sn is lower than that of Zn, meaning Sn is not strong enough to reduce Zn in this scenario.
What type of reaction is N2H4 plus 3O2 equals 2NO2 plus 2H2O?
This is an oxidation-reduction reaction.
