Answer:
See below
Explanation:
Use Ideal Gas Law
PV = n RT using R = .082057366 l-atm/k-mol
T must be in Kelvin
solve for 'n'
.92 * 1.6 = n * .082057366 * 287
n = .0625 moles
then the mole weight: .0625 * x = .314
x = mole weight = 5.025 gm
"Systems with either very low pressures or high temperatures enable real gases to be estimated as “ideal.” "
The ideal gas equation estimates the molar mass of the substance with the help of the moles. The molar mass of 0.314 gm sample and 1.6 L volume is 0.503g/mol.
The gas is said to be ideal at low pressure, and high-temperature conditions as the potential energy and the molecular size become negligible because of the intermolecular forces.
The ideal gas equation is given as,
PV = nRT
Given,
Pressure (P) = 0.92 atm
Volume (V) = 1.6 L
Gas law constant (R) = 0.0821
Temperature (T) = 287 K
Mass of sample = 0.314 gram
No. of moles = n
The moles are calculated as:
PV = nRT
0.92 × 1.6 = n × 0.0821 × 287
1.47 = 23.56 × n
n = 1.47 ÷ 23.56
n = 0.624 moles
Now, from moles, the molar mass is calculated as,
Molar mass = mass ÷ moles
Molar mass = 0.314g ÷ 0.624mol
Molar mass = 0.503 g/mol
Therefore, 0.503g/mol is the molar mass of the 0.314 gm sample.
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