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Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy ΔG0 for the following redox reaction. Round your answer to 3 significant digits. 10Cl^(−)(aq) + 2MnO4^(−)(aq) + 16H^(+)(aq) = 5Cl2(g) + 2Mn^(+2)(aq) + 8H2O(l)

Respuesta :

Answer:

The standard reaction free energy = -144 kj

Explanation:

According to Electrochemical series

Standard reduction potential of

  1. Cl₂  + 2 e⁻  → 2 Cl⁻                                 E⁰ = +1.36 volt .................(i)
  2. MnO₄⁻ + 8H⁺ + 5 e⁻ → Mn²⁺  + 4 H₂O   E⁰ = +1.51 volt ..................(ii)

Since Permanganate have more positive reduction potential so it is used as a cathode half cell and chlorine as a anode half cell

Cathode half cell (Reduction)     MnO₄⁻ + 8H⁺ + 5 e⁻ → Mn²⁺  + 4 H₂O ...(3)

Anode half cell    (Oxidation)       2 Cl⁻    →   Cl₂  + 2 e⁻ ...............................(4)

Multiplication by 2 of equation (3) and by 5 of equation(4)

10Cl⁻(aq) + 2MnO₄⁻(aq) + 16H⁺(aq) = 5Cl₂(g) + 2Mn²⁺(aq) + 8H₂O(l)

E.M.F of the combined cell reaction

                 E⁰ = E⁰cathode - E⁰anode = 1.51 - 1.36 = 0.15 v

               ⇒ ΔG⁰ reaction = - nF E⁰cell

n = no, of electron exchange = 10

              ⇒ΔG⁰ reaction = - 10 x 96500 x 0.15

                                        = - 144750 j

                                        = - 144 kj (round off by 3 significant fig.)

dsdrajlin

The standard Gibbs free energy for the given redox reaction is -106 kJ/mol.

Let's consider the following redox reaction.

10 Cl⁻(aq) + 2 MnO₄⁻(aq) + 16 H⁺(aq) ⇒ 5 Cl₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)

We can identify both half-reactions with their respective standard reduction potentials (E°red).

Cathode: 2 MnO₄⁻ + 16 H⁺ + 10 e⁻ ⇒ 2 Mn²⁺ + 8 H₂O  E°red = 1.51 V

Anode: 10 Cl⁻ ⇒ 5 Cl₂ + 10 e⁻                                        E°red = 1.40 V

With this information, we will calculate the standard cell potential (E°cell).

What is the standard cell potential?

The standard cell potential is the potential difference between the cathode and anode.

E°cell = Ered,cathode - E°red,anode = 1.51 V - 1.40 V = 0.11 V

What is the standard Gibbs free energy?

The standard Gibbs free energy (ΔG°) is a thermodynamic potential that can be used to calculate the maximum reversible work that may be performed by a thermodynamic system under standard conditions.

It can be calculated using the following expression

ΔG° = - n × F × E°cell

ΔG° = - 10 mol × (96,485 J/V.mol) × 0.11 V × (1 kJ/1000 J) = -106 kJ/mol

where,

  • n are the moles of electrons exchanged.
  • F is Faraday's constant.

The standard Gibbs free energy for the given redox reaction is -106 kJ/mol.

Learn more about standard Gibbs free energy here: https://brainly.com/question/10012881

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