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Two moles of helium gas initially at 321 K
and 0.42 atm are compressed isothermally to
1.83 atm.
Find the final volume of the gas. Assume
that helium behaves as an ideal gas. The
universal gas constant is 8.31451 J/K·mol.
Answer in units of m^3

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nuhulawal20

If the helium behaves as an ideal gas, its final volume is 0.13m³.

Ideal Gas Law

The ideal gas law states "that pressure multiplied by volume is equal to moles multiply by the universal gas constant multiply by temperature of gas. It is expressed;

PV = nRT

Where P is pressure, V is volume, n is the amount of substance, T is temperature and R is the ideal gas constant.

Given the data in the question;

  • Amount of helium gas; n = 2mol
  • Temperature T = 321K
  • Pressure P = 0.42atm = 42556.5Pa
  • Universal gas constant R = 8.31451 J/K·mol = 8.31451 m³Pa/Kmol
  • Volume V = ?

To determine the volume of the helium gas, we substitute our given values into the expression above.

PV = nRT

V = nRT / P

V = ( 2mol × 8.31451 m³Pa/Kmol × 321K ) / 42556.5Pa

V = 5337.91542m³Pa / 42556.5Pa

V = 0.13m³

Therefore, if the helium behaves as an ideal gas, its final volume is 0.13m³

Learn more about Ideal gas law here: brainly.com/question/4147359

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