A 2.36 g sample of an imaginary gas occupies a volume of 890 mL at 39.6 oC and 114 kPa. Determine the molar mass of the compound.
(Hint: molar mass can be found by dividing a mass by a number of mole)
** MAKE SURE TO HAVE THE CORRECT SIGNIFICANT DIGITS **
The molar mass of this imaginary gas is g/mol.
To find the molar mass of the gas, we first need to calculate the number of moles present in the sample using the ideal gas law equation:
PV = nRT
where:
P = pressure (114 kPa)
V = volume (890 mL = 0.89 L)
n = number of moles
R = ideal gas constant (8.31 L*kPa/mol*K)
T = temperature (39.6 oC = 312.75 K)
Rearranging the equation to solve for n:
n = (PV)/(RT)
n = (114 kPa * 0.89 L) / (8.31 L*kPa/mol*K * 312.75 K)
n = 0.03934 moles
Now that we have the number of moles, we can find the molar mass of the gas by dividing the mass of the sample by the number of moles:
Molar mass = (2.36 g) / (0.03934 mol)
Molar mass = 59.9 g/mol
Therefore, the molar mass of the imaginary gas is 59.9 g/mol.