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A sample of gas has a mass of 38.6 mg. Its volume is 222 mL at a temperature of 57 ∘C and a pressure of 918 torr.

Find the molar mass of the gas.

Answer :

The molar mass of the gas is 3.58 g/mol.

To find the molar mass of the gas

We can use the ideal gas law equation:

[tex]PV = nRT[/tex]

Where

  • P is the pressure in torr
  • volume (in milliliters)
  • The number of moles is n
  • R = 62.36 L torr/mol K, the ideal gas constant
  • T is the temperature (in K)

We can rearrange the equation to solve for n:

[tex]n = PV/RT[/tex]

We know the following values:

P = 918 torr

V = 222 mL

R = 62.36 L torr/mol K

T = 57°C + 273 = 330 K

To solve for n, we can enter these numbers into the equation:

n = (918 torr)(222 mL)/(62.36 L torr/mol K)(330 K) = 0.0108 mol

Now, we can use the definition of molar mass to find the molar mass of the gas:

molar mass = mass/number of moles

We know the following values:

mass = 38.6 mg = 0.0386 g

n = 0.0108 mol

We can plug these values into the equation to solve for the molar mass

molar mass = 0.0386 g/0.0108 mol = 3.58 g/mol

Therefore, the molar mass of the gas is 3.58 g/mol.

Learn more about ideal gas law here : brainly.com/question/12873752

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