Question
Asked Oct 28, 2019
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A 1.95 g sample of an unknown gas at 61 ∘C and 1.00 atm is stored in a 1.45 L flask.

What is the molar mass of the gas?
A 1.95 g sample of an unknown gas at 61 °C and 1.00 atm is stored in a 1.45 L flask.
What is the density of the gas?
density: 1.34
g/L
What is the molar mass of the gas?
molar mass:
36.86
g/mol
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A 1.95 g sample of an unknown gas at 61 °C and 1.00 atm is stored in a 1.45 L flask. What is the density of the gas? density: 1.34 g/L What is the molar mass of the gas? molar mass: 36.86 g/mol

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Expert Answer

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Step 1

Given information:

Mass of sample = 1.95 g

Temperature = 61 °C

Pressure of gas = 1.00 atm

Volume of flask = 1.45 L

Step 2

Ideal gas law gives the empirical relationship between pressure, volume, temperature, and amount of gas that is number of moles of a gas. The ideal gas equation is represented as follows:

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pV nRT where,Pispressure of the gas Visvolumeoccupied by the gas nisnumber of moles of the gas Risproportionality constant(Universalgas constant having a value 0.082 1L. atm/mol.K) Tis thetemperature

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Step 3

As, the temperature of gas is given in degree Celsius so,...

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61° C+273.15 K T =334.15 K

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Science

Chemistry

Gas laws

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