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MMLU-Pro / 4361 / Assume all gases are perfect unless stated otherwise. Note that 1 atm = 1.013 25…

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question

Assume all gases are perfect unless stated otherwise. Note that 1 atm = 1.013 25 bar. Unless otherwise stated, thermochemical data are for 298.15 K. Silylene (SiH2)\left(\mathrm{SiH}_2\right) is a key intermediate in the thermal decomposition of silicon hydrides such as silane (SiH4)\left(\mathrm{SiH}_4\right) and disilane (Si2H6)\left(\mathrm{Si}_2 \mathrm{H}_6\right). Moffat et al. (J. Phys. Chem. 95, 145 (1991)) report $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{SiH}_2\right)=+274 \mathrm{~kJ} \mathrm{~mol}^{-1}$. If $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{SiH}_4\right)=+34.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{Si}_2 \mathrm{H}_6\right)=+80.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$(CRC Handbook (2008)), compute the standard enthalpies of the following reaction: SiH4(g)→SiH2(g)+H2(g)\mathrm{SiH}_4 (\mathrm{g}) \rightarrow \mathrm{SiH}_2(\mathrm{g})+\mathrm{H}_2(\mathrm{g})
Plain-text mathematical notation (without MathML)
Assume all gases are perfect unless stated otherwise. Note that 1 atm = 1.013 25 bar. Unless otherwise stated, thermochemical data are for 298.15 K.
Silylene (SiH₂) is a key intermediate in the thermal decomposition of silicon hydrides such as silane (SiH₄) and disilane (Si₂H₆). Moffat et al. (J. Phys. Chem. 95, 145 (1991)) report $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{SiH}_2\right)=+274 \mathrm{~kJ} \mathrm{~mol}^{-1}$. If $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{SiH}_4\right)=+34.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{Si}_2 \mathrm{H}_6\right)=+80.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$(CRC Handbook (2008)), compute the standard enthalpies of the following reaction:
SiH₄(g)→SiH₂(g)+H₂(g)
Original LaTeX notation
Assume all gases are perfect unless stated otherwise. Note that 1 atm = 1.013 25 bar. Unless otherwise stated, thermochemical data are for 298.15 K.
Silylene $\left(\mathrm{SiH}_2\right)$ is a key intermediate in the thermal decomposition of silicon hydrides such as silane $\left(\mathrm{SiH}_4\right)$ and disilane $\left(\mathrm{Si}_2 \mathrm{H}_6\right)$. Moffat et al. (J. Phys. Chem. 95, 145 (1991)) report $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{SiH}_2\right)=+274 \mathrm{~kJ} \mathrm{~mol}^{-1}$. If $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{SiH}_4\right)=+34.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$ and $\Delta_{\mathrm{f}} H^{\ominus}\left(\mathrm{Si}_2 \mathrm{H}_6\right)=+80.3 \mathrm{~kJ} \mathrm{~mol}^{-1}$(CRC Handbook (2008)), compute the standard enthalpies of the following reaction:
$\mathrm{SiH}_4 (\mathrm{g}) \rightarrow \mathrm{SiH}_2(\mathrm{g})+\mathrm{H}_2(\mathrm{g})$

category

chemistry

options

  1. 330 kJ mol^{-1}
  2. 255 kJ mol^{-1}
  3. 180$\mathrm{kJ} \mathrm{mol}^{-1}$
  4. 150 kJ mol^{-1}
  5. 240$\mathrm{kJ} \mathrm{mol}^{-1}$
  6. 270 kJ mol^{-1}
  7. 300$\mathrm{kJ} \mathrm{mol}^{-1}$
  8. 120 kJ mol^{-1}
  9. 195 kJ mol^{-1}
  10. 210$\mathrm{kJ} \mathrm{mol}^{-1}$

src

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Source and history

upstream_id / Original problem ID
4361
task_id
cf076438-897e-5946-8e3f-0205e6593120
task_key
default--test--4361
task_revision_id
1
config / split
default / test

Official source

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