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Oksanka [162]
3 years ago
6

A 2.00 liter evacuated container has a mass of 1050.0 g. When the container is filled with an unknown gas at 800. mm Hg pressure

and 25.0 °C the mass is 1052.4 g. What is the molar mass of the gas (in g-mol"')?
(A) 28
(B) 31
(C) 54
(D) 56
Chemistry
1 answer:
Andrei [34K]3 years ago
5 0

Answer:

(A) 28

Explanation:

To solve this problem we use the <em>PV=nRT equation</em>, where:

  • P = 800 mmHg ⇒ 800/760 = 1.05 atm
  • V = 2.00 L
  • n = ?
  • R = 0.082 atm·L·mol⁻¹·K⁻¹
  • T = 25.0 °C ⇒ 25.0 + 273.16 = 298.16 K

We<u> input the data</u>:

  • 1.05 atm * 2.00 L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 298.16 K

And <u>solve for n</u>:

  • n = 0.086 mol

Now we calculate the gas' mass:

  • Gas Mass = (Mass of Container w/ Gas) - (Mass of Empty Container)
  • Gas Mass = 1052.4 g - 1050.0 g = 2.4 g

Finally we <u>calculate the unknown gas' molar mas</u>s, using<em> its mass and its number of moles</em>:

  • Molar Mass = mass / moles
  • Molar Mass = 2.4 g / 0.086 mol = 27.9 g/mol

So the answer is option (A).

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In this case, according to the given information, it turns out necessary for us to bear to mind the definition of each type of solution:

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