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Montano1993 [528]
3 years ago
13

A voltaic electrochemical cell consists of a copper electrode in a Cu2SO4(aq) solution, and a palladium electrode in a PdSO4(aq)

solution at 25°C. The salt bridge consists of a solution of KCl(aq).
What is the concentration of the Cu+if the concentration of the PdSO4 is 0.498 M and the measured cell potential is 0.447 V?

Given: Cu+(aq) + e- ↔ Cu(s) E°=+0.521 V

and Pd2+(aq) + 2e- ↔ Pd(s) E°=+0.987 V
Chemistry
1 answer:
lianna [129]3 years ago
8 0

Answer:

\large \boxed{\textbf{1.48 mol/L}}

Explanation:

We must use the Nernst equation

E = E^{\circ} - \dfrac{RT}{zF}lnQ

1. Calculate E°

Anode:     Pd²⁺ (0.498 mol·L⁻¹) + 2e⁻ ⇌ Pd;                               E° = +0.987 V

<u>Cathode: Cu ⇌ Cu⁺ (x mol·L⁻¹) + e⁻;                                         </u>  E°=  <u>- 0.521 V </u>

Overall:   Pd²⁺(0.498 mol·L⁻¹) + 2Cu ⟶ Pd + 2Cu⁺ (x mol·L⁻¹); E° =   0.466 V

2. Calculate Q

\begin{array}{rcl}0.447 & = & 0.466 - \dfrac{8.314\times 298}{2 \times 96 485} \ln Q\\\\-0.019& = & -0.01284 \ln Q\\\ln Q & = & 1.480\\Q & = & e^{1.480}\\ & = & 4.392\\\end{array}

3. Calculate [Cu⁺]

\begin{array}{rcl}Q & = & \dfrac{\text{[Cu$^{+}$]}^{2}}{\text{[Pd]}}\\\\4.392 & = & \dfrac{{x}^{2}}{0.498}\\\\x^{2}& = & 2.187\\x & = & 1.48\\\end{array}\\\text{The concentration of Cu$^{+}$ is $\large \boxed{\textbf{1.48 mol/L}}$}

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The mole fraction of a non-electrolyte (MM 40.0 g/mol) in a saturated aqueous solution is 0.310. What is the molality of the sol
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<u>Answer:</u> The molality of non-electrolyte is 24.69 m

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Mole fraction of saturated aqueous solution = 0.310

This means that 0.310 moles of non-electrolyte is present.

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To calculate the mass from given number of moles, we use the equation:

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Moles of water = 0.690 moles

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Putting values in above equation, we get:

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To calculate the molality of solution, we use the equation:

\text{Molality}=\frac{n_{solute}\times 1000}{W_{solvent}\text{ (in grams)}}

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Putting values in above equation, we get:

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