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2.58g of a gas has a volume of 3.97L at 745 mmHg and 21°C determine the molar mass of the gas what might be? ( first find n from the ideal gas law equation; then plug it into N = m/M or M = m/n)

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Nuhulawal20idn

The molar mass of the gas with the given mass and volume at the given temperature and pressure is 16.00g/mol.

What is the molar mass of the gas?

From the Ideal gas law or general gas equation;

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 ( 0.08206 Latm/molK )

Given that;

  • Temperature T = 21°C = (21 + 273.15)K = 294.15K
  • Pressure P = 745 mmHg = (745/760)atm = 0.98026atm
  • Volume of the gas V = 3.97L
  • Mass of gas m = 2.58g
  • Amount of gas n = ?

First, we determine the amount of gas;

PV = nRT

n = PV / RT

n = ( 0.98026atm × 3.97L ) / ( 0.08206 Latm/molK × 294.15K )

n = 3.8916Latm / (24.137949Latm/mol)

n = 0.1612mol

Molar Mass = Mass of the gas / Amount of the gas

Molar Mass = m / n

Molar Mass = 2.58g / 0.1612mol

Molar Mass = 16.00g/mol

Therefore, the molar mass of the gas with the given mass and volume at the given temperature and pressure is 16.00g/mol.

Learn more about ideal gases here: brainly.com/question/15634266

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