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青州's Question
Posted 3 months ago

6. A. Calculate the potential of the cell where the reaction: 2 \mathrm{HClO}_{2} 3 / 4 ® \mathrm{HClO}^{3}+\mathrm{ClO}_{3}-+\mathrm{H}^{+} occurs if: [HClO2]=0.01M;[HClO]=0.10M;[ClO3]=0.10M\left[\mathrm{HClO}_{2}\right]=0.01 \mathrm{M} ;[\mathrm{HClO}]=0.10 \mathrm{M} ;\left[\mathrm{ClO}_{3}-\right]=0.10 \mathrm{M} and pH=5.0\mathrm{pH}=5.0
B. Taking all species to be 1M1 \mathrm{M} except HClO2\mathrm{HClO}_{2}, calculate the concentration of HClO2\mathrm{HClO}_{2} at which the reaction would no longer be spontaneous.
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Answer from Sia
Posted 3 months ago
Write the balanced half-reactions and the overall reaction: The given reaction is not balanced. We need to balance it in terms of atoms and charges to use it in further calculations
Calculate the standard cell potential (E°): The standard cell potential is calculated using the standard reduction potentials of the half-reactions. However, since the standard reduction potentials are not provided, we will assume that the Nernst equation will be used to calculate the cell potential under non-standard conditions
Use the Nernst equation: The Nernst equation relates the cell potential to the standard cell potential and the reaction quotient (Q). The equation is E=E°0.0592nlogQE = E° - \frac{0.0592}{n} \log Q, where nn is the number of moles of electrons transferred in the balanced equation, and QQ is the reaction quotient
Calculate the reaction quotient (Q): For the reaction 2HClO2HClO+ClO3+H+2 \mathrm{HClO}_{2} \rightarrow \mathrm{HClO} + \mathrm{ClO}_{3}^{-} + \mathrm{H}^{+}, the reaction quotient QQ is given by Q=[HClO][ClO3][H+][HClO2]2Q = \frac{[\mathrm{HClO}][\mathrm{ClO}_{3}^{-}][\mathrm{H}^{+}]}{[\mathrm{HClO}_{2}]^2}. We can calculate QQ using the given concentrations and the pH of the solution
Calculate the pH and the concentration of $\mathrm{H}^{+}$: The pH is given as 5.0, which means the concentration of H+\mathrm{H}^{+} is 105M10^{-5} \mathrm{M}
Plug the values into the Nernst equation: Substitute the calculated values of QQ and the concentration of H+\mathrm{H}^{+} into the Nernst equation to find the cell potential EE
Determine the spontaneity condition: For a reaction to be spontaneous, the cell potential EE must be positive. To find the concentration of HClO2\mathrm{HClO}_{2} at which the reaction is no longer spontaneous, we set EE to zero and solve for [HClO2][\mathrm{HClO}_{2}]
A Answer
[Insert final answer for part A here]
B Answer
[Insert final answer for part B here]
Key Concept
The Nernst equation is used to calculate the cell potential under non-standard conditions and determine the spontaneity of a reaction.
The Nernst equation allows us to relate the cell potential to the concentrations of the reactants and products. By knowing the cell potential, we can predict whether a reaction will occur spontaneously under given conditions.

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