determine whether each reaction is likely to occur spontaneously under standard conditions: a. Sn(s) + Be2+(aq) → Sn2+(aq) + Be(s) b. MnO2(s) + H2O2(aq) + 2H+ (aq) → O2(g) + Mn2+(aq) + 2H2O(l)

Q: The following reactions are used in batteries:I 2H₂(g)+ O₂(g) → 2H₂O(l) E(cell)=1.23 V II Pb(s)…

A: (a)

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A: The given unbalanced redox reaction is: F-+HgO→Hg+F2

Q: Complete and balance the following half-reaction in acidic solution. Be sure to include the proper…

A:

Q: lance each redox reaction. Label the half reactions as oxidation or reduction and identify the…

A: Balanced redox reaction:

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A: Oxidation reduction reactions are those in which oxidation and reduction of atoms take place.…

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A: Loss of electrons is oxidation and loss of electrons is reduction.  Reduction half reaction = 3e +…

Q: Write the balanced reaction for the following half reactions. Specify whether it is an oxidation or…

A: Given reaction balancing  a.) Reaction [Acidic medium] Cr(s)  → Cr+3(aq.)    (acidic medium) Cr(s) →…

Q: Consider the following balanced redox reaction:               16H+(aq) + 2MnO4-(aq) + 10Cl-(aq) →…

A: Species whose oxidation occur is called reducing agent and the species whose reduction occur is…

Q: 6. Consider the following half-reactions: F2(g) +2 e-→2 F-(aq) Cu2*(aq)+2 e-→ Cu(s) Sn²*(aq)+2 e –→…

A: The reducing agent is the substance that causes other substance to reduce while the oxidizing agent…

Q: Balance the following redox reaction in basic solution: MnO4 (aq) + Br (aq) MnO2(s) + BRO3 (aq) What…

A: Balance the Redox reaction by oxidation number method.  First balance increase and decrease in…

Q: Calculate the cell potential for the reaction as written at 25.00 °C, given that [Zn²+] = 0.867 M…

A:

Q: Use the following standard reduction potentials to determine which species is the strongest…

A: Oxidizing agent oxidizes other substance and reduced itself. Strongest oxidizing agent has the half…

Q: rite the half-reaction equations. 2Als) + 3B12(1) → 2AIB13(9) Number

A: Oxidation number of reactants Al = 0 Br = 0 Products  Al = +3 Br = -1 Oxidized = Al Reduced = Br2

Q: ance the following reaction in basic solution. l in the coefficients for the balanced overall…

A: We have to balance the given equation

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A:

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Q: calculate the standard free energy change (kJ) for the reaction at 25°C. use the standard reduction…

A: ∆G° = -nFE°  n = number of electrons involved  F = Faraday constant  E° = standard emf