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Problem

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question

N2O3\mathrm{N}_2 \mathrm{O}_3 dissociates according to the equilibrium $\mathrm{N}_2 \mathrm{O}_3(\mathrm{~g}) \rightleftharpoons \mathrm{NO}_2(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$. At $298 \mathrm{~K}$ and one bar pressure, the degree of dissociation defined as the ratio of moles of NO2(g)\mathrm{NO}_2(g) or NO(g)\mathrm{NO}(g) to the moles of the reactant assuming no dissociation occurs is 3.5×10−33.5 \times 10^{-3}. Calculate ΔGR∘\Delta G_R^{\circ} for this reaction.
Plain-text mathematical notation (without MathML)
N₂O₃ dissociates according to the equilibrium $\mathrm{N}_2 \mathrm{O}_3(\mathrm{~g}) \rightleftharpoons \mathrm{NO}_2(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$. At $298 \mathrm{~K}$ and one bar pressure, the degree of dissociation defined as the ratio of moles of NO₂(g) or NO(g) to the moles of the reactant assuming no dissociation occurs is 3.5×10^(−3). Calculate ΔG_(R)^(∘) for this reaction.
Original LaTeX notation
$\mathrm{N}_2 \mathrm{O}_3$ dissociates according to the equilibrium $\mathrm{N}_2 \mathrm{O}_3(\mathrm{~g}) \rightleftharpoons \mathrm{NO}_2(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$. At $298 \mathrm{~K}$ and one bar pressure, the degree of dissociation defined as the ratio of moles of $\mathrm{NO}_2(g)$ or $\mathrm{NO}(g)$ to the moles of the reactant assuming no dissociation occurs is $3.5 \times 10^{-3}$. Calculate $\Delta G_R^{\circ}$ for this reaction.

category

physics

options

  1. 14 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  2. 42 kJ mol^{-1}
  3. 56 kJ mol^{-1}
  4. 50 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  5. 5 kJ mol^{-1}
  6. 75 kJ mol^{-1}
  7. 28 $\mathrm{~kJ} \mathrm{~mol}^{-1}$
  8. 21 kJ mol^{-1}
  9. 65 kJ mol^{-1}
  10. 35 $\mathrm{~kJ} \mathrm{~mol}^{-1}$

src

scibench-thermo

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Source and history

Official source

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