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MMLU-Pro / 9061 / Consider the half-cell reaction …

Problem

Answer published by the source. Consult the official source to check your work against its answer.

question

Consider the half-cell reaction AgCl(s)+e−→\operatorname{AgCl}(s)+\mathrm{e}^{-} \rightarrow Ag(s)+Cl−(aq)\operatorname{Ag}(s)+\mathrm{Cl}^{-}(a q). If $\mu^{\circ}(\mathrm{AgCl}, s)=-109.71 \mathrm{~kJ} \mathrm{~mol}^{-1}$, and if $E^{\circ}=+0.222 \mathrm{~V}$ for this half-cell, calculate the standard Gibbs energy of formation of Cl−(aq)\mathrm{Cl}^{-}(a q).
Plain-text mathematical notation (without MathML)
Consider the half-cell reaction AgCl(s)+e^(−)→ Ag(s)+Cl^(−)(aq). If $\mu^{\circ}(\mathrm{AgCl}, s)=-109.71 \mathrm{~kJ} \mathrm{~mol}^{-1}$, and if $E^{\circ}=+0.222 \mathrm{~V}$ for this half-cell, calculate the standard Gibbs energy of formation of Cl^(−)(aq).
Original LaTeX notation
Consider the half-cell reaction $\operatorname{AgCl}(s)+\mathrm{e}^{-} \rightarrow$ $\operatorname{Ag}(s)+\mathrm{Cl}^{-}(a q)$. If $\mu^{\circ}(\mathrm{AgCl}, s)=-109.71 \mathrm{~kJ} \mathrm{~mol}^{-1}$, and if $E^{\circ}=+0.222 \mathrm{~V}$ for this half-cell, calculate the standard Gibbs energy of formation of $\mathrm{Cl}^{-}(a q)$.

category

physics

options

  1. -137.5 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  2. -140.9 kJ mol^{-1}
  3. -131.1 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  4. -145.2 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  5. -122.7 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  6. -128.4 kJ mol^{-1}
  7. -155.7 kJ mol^{-1}
  8. -150.3 kJ mol^{-1}
  9. -100.0 kJ mol^{-1}
  10. -115.6 kJ mol^{-1}

src

scibench-thermo

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Source and history

upstream_id / Original problem ID
9061
task_id
75cc1db8-ec1e-53c8-a569-f76305a1f733
task_key
default--test--9061
task_revision_id
1
config / split
default / test

Official source

initial import