Question

Be sure to answer all parts. calculate δg ocell for the reaction between cr(s) and cu2+(aq). e ocell = 1.08 j/c. enter your answer in scientific notation. δg ocell = × 10 j

Answer 1

Answer:

$\boxed{-6.29 \times10^{5}\text{ J}}$

Explanation:

Step 1. Determine the cell potential

                                                     E°/V    

2×[Cr ⟶ Cr³⁺ + 3e⁻]                  0.744  V

3×[Cu²⁺ + 2e⁻ ⟶ Cu]               0.3419 V

2Cr + 3Cu²⁺ ⟶ 3Cu  + 2Cr³⁺    1.086  V

Step 2. Calculate ΔG°

$\Delta G^{\circ} = -nFE_{\text{cell}}^{^{\circ}} = -6 \times 96 485 \times 1.086 = \text{-629 000 J}\\\\= \boxed{-6.29 \times10^{5}\text{ J}}$

Answer 2

The value of change in free energy of the given cell reaction is -6.2×10⁵J.

How do we calculate the ΔG for the cell?

Change in free energy for a cell will be calculated by using the below equation as:

ΔG° = -nFE°, where

• n = number of electrons
• F = faradays constant = 96485
• E° = electrode potential = 1.08 J/C

2×[Cr ⟶ Cr³⁺ + 3e⁻]              

3×[Cu²⁺ + 2e⁻ ⟶ Cu]            

Overall reaction will be

2Cr + 3Cu²⁺ ⟶ 3Cu  + 2Cr³⁺

So number of electrons involved are 6.

On putting all these values on the above equation, we get

ΔG° = -(6)(96485)(1.08) = -625,222.8J = -6.2×10⁵J

Hence required value of ΔG° for the cell is -6.2×10⁵J.

To now more about electrode potential, visit the below link:

https://brainly.com/question/8655719

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