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Question 41
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A 1.00-mole sample of neon gas occupies a volume of 24.4 liters at 298 K and 101.3 kilopascals. Which numerical setup can be used to calculate the density of this sample?
20.1798
1 mole
20.179 8
2241
20.179 1
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Answer 1

d = 0.9 g/L

Step-by-step explanation:

Given data:

Number of moles = 1 mol

Volume = 24.2 L

Temperature = 298 K

Pressure = 101.3 Kpa (101.3/101 = 1 atm)

Density of sample = ?

Solution:

PV = nRT (1)

n = number of moles

number of moles = mass/molar mass

n = m/M

Now we will put the n= m/M in equation 1.

PV = m/M RT (2)

d = m/v

PM = m/v RT ( by rearranging the equation 2)

PM = dRT

d = PM/RT

The molar mass of neon is = 20.1798 g/mol

d = 1 atm × 20.1798 g/mol / 0.0821 atm. L/mol.K × 273K

d = 20.1798 g/22.413 L

d = 0.9 g/L