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MMLU-Pro / 4275 / In an industrial process, nitrogen is heated to 500 mathrm{~K} at a constant…

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question

In an industrial process, nitrogen is heated to $500 \mathrm{~K}$ at a constant volume of $1.000 \mathrm{~m}^3$. The gas enters the container at $300 \mathrm{~K}$ and $100 \mathrm{~atm}$. The mass of the gas is $92.4 \mathrm{~kg}$. Use the van der Waals equation to determine the approximate pressure of the gas at its working temperature of $500 \mathrm{~K}$. For nitrogen, $a=1.352 \mathrm{dm}^6 \mathrm{~atm} \mathrm{~mol}^{-2}, b=0.0387 \mathrm{dm}^3 \mathrm{~mol}^{-1}$.
Plain-text mathematical notation (without MathML)
In an industrial process, nitrogen is heated to $500 \mathrm{~K}$ at a constant volume of $1.000 \mathrm{~m}^3$. The gas enters the container at $300 \mathrm{~K}$ and $100 \mathrm{~atm}$. The mass of the gas is $92.4 \mathrm{~kg}$. Use the van der Waals equation to determine the approximate pressure of the gas at its working temperature of $500 \mathrm{~K}$. For nitrogen, $a=1.352 \mathrm{dm}^6 \mathrm{~atm} \mathrm{~mol}^{-2}, b=0.0387 \mathrm{dm}^3 \mathrm{~mol}^{-1}$.
Original LaTeX notation
In an industrial process, nitrogen is heated to $500 \mathrm{~K}$ at a constant volume of $1.000 \mathrm{~m}^3$. The gas enters the container at $300 \mathrm{~K}$ and $100 \mathrm{~atm}$. The mass of the gas is $92.4 \mathrm{~kg}$. Use the van der Waals equation to determine the approximate pressure of the gas at its working temperature of $500 \mathrm{~K}$. For nitrogen, $a=1.352 \mathrm{dm}^6 \mathrm{~atm} \mathrm{~mol}^{-2}, b=0.0387 \mathrm{dm}^3 \mathrm{~mol}^{-1}$.

category

chemistry

options

  1. 140$\text{atm}$
  2. 130$\text{atm}$
  3. 120$\text{atm}$
  4. 150$\text{atm}$
  5. 180$\text{atm}$
  6. 110$\text{atm}$
  7. 170$\text{atm}$
  8. 220$\text{atm}$
  9. 160$\text{atm}$
  10. 200$\text{atm}$

src

scibench-atkins

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Official source

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