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The mass of a flask with a 1L volume that is evacuated to a pressure of 0.00 atm is found to be 92.01g. after introduction of an unknown ideal gas with a pressure of 3.00 atm and temprature of 27 Degrees C the mass of the flask and gas are found to be 97.37g. Identify the unknown gas.

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Answer:

CO₂

Explanation:

We substract the mass of the empty flask from the mass of the flask + gas in order to calculate the mass of the gas:

  • 97.37 g - 92.01 g = 5.36 g

The moles of this gas (n) can be expressed as:

  • n = 5.36 g ÷ M

Where M is the molar mass.

We can calculate n using PV=nRT:

  • P = 3.00 atm
  • V = 1 L
  • T = 27 °C ⇒ 27+273.16 = 300.16 K

3.00 atm * 1L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 300.16 K

  • n = 0.122 mol

Now we can calculate the molar mass of the gas:

n = 5.36 g ÷ M

  • 0.122mol = 5.36 g ÷ M
  • M = 43.9 g/mol ≅ 44 g/mol

Thus, the gas is most likely CO₂.

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