The density of a gaseous compound was found to be 0.963 g·L-1 at 275 K and 51.6 kPa. What is the molar mass of the compound?
Please explain. Thanks :)
Start with the ideal gas equation
PV = nRT
we know that moles (n) = mass (m) / molar mass (M)
substitute this into the equation and we get
PV = mRT / M
Now, we also know that density (d) = mass (m) / volume (V)
so rearrange the modified gas equation such that m/V (density) is on one side by itself
m/V = PM / RT
density = PM / RT
P = pressure = 51.6 kPa
M = molar mass = ? g/mol
R = gas constant = 8.3145 kPa L mol^-1 K^-1
T = temp in Kelvin = 275 K
density (d) = 0.963 g/L
solve for M
M = dRT / P
= 0.963 gL^-1 x 8.3145 kPaLmol^-1K^-1 x 275 K / 51.6 kPa
= 42.7 g/mol (3 sig figs)
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Verified answer
Start with the ideal gas equation
PV = nRT
we know that moles (n) = mass (m) / molar mass (M)
substitute this into the equation and we get
PV = mRT / M
Now, we also know that density (d) = mass (m) / volume (V)
so rearrange the modified gas equation such that m/V (density) is on one side by itself
m/V = PM / RT
density = PM / RT
P = pressure = 51.6 kPa
M = molar mass = ? g/mol
R = gas constant = 8.3145 kPa L mol^-1 K^-1
T = temp in Kelvin = 275 K
density (d) = 0.963 g/L
solve for M
M = dRT / P
= 0.963 gL^-1 x 8.3145 kPaLmol^-1K^-1 x 275 K / 51.6 kPa
= 42.7 g/mol (3 sig figs)