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In an experiment, a liquid was vaporized in an Erlenmeyer flask, which had a total volume of 165 mL, at 100 °C and 0.9921 atm of pressure. The mass of vapor in the flask was determined to be 0.38 grams. What is the molecular weight of this volatile liquid?

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The molar mass can be obtained from the number of moles of the gas. The molar mass of the gas is 70.3 g/mol.

We have to use the ideal gas equation;

PV = nRT

P = 0.9921 atm

V = 165 mL or 0.165 L

n = ?

R = 0.082 atmLK-1mol-1

T =  100 °C + 273 = 373 K

Now we have to find the number of moles (n)

n = PV/RT

n =  0.9921 atm × 0.165 L/0.082 atmLK-1mol-1 × 373 K

n = 0.164/30.6

n = 0.0054 moles

Since, number of moles = mass/molar mass

molar mass = 0.38g/0.0054 moles = 70.3 g/mol

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