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An ideal gas at 15.5oC and a pressure of 1.72 x 10^5 Pa occupies a volume of 2.81 m3. How many moles of gas are present?

Correct answer: C. 201 mol

  • A. 2.01 mol
  • B. 21 mol
  • C. 201 mol
  • D. 2001 mol

Explanation

Using the ideal gas equation PV = nRT, we can solve for n:n = PV / RTGiven:P = 1.72 x 10^5 PaV = 2.81 m^3R = 8.314 J/(mol K)T = 15.5°C = 15.5 + 273.15 = 288.65 KSubstituting the values:n = (1.72 x 10^5 Pa) * (2.81 m^3) / (8.314 J/(mol K) * 288.65 K)Calculating:n ≈ 201.6 molTherefore, the correct answer is approximately 201.6 mol, which is closest to option C) 201 mol.

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