A 1.21 g sample of an imaginary gas occupies a volume of 860 mL at 43.0 oC and 113 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.
A 1.21 g sample of an imaginary gas occupies a volume of 860 mL at 43.0 oC and 113 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 compound, we first need to calculate the number of moles of the gas using the ideal gas law:
PV = nRT
where:
P = pressure (113 kPa = 113000 Pa)
V = volume (860 mL = 0.86 L)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature in Kelvin (273.15 + 43.0 = 316.15 K)
Now, rearranging the equation to solve for n:
n = (PV) / (RT)
n = (113000 Pa * 0.86 L) / (8.314 J/(mol·K) * 316.15 K)
n = 0.102 moles
Next, we can calculate the molar mass by dividing the mass of the compound by the number of moles:
molar mass = 1.21 g / 0.102 mol
molar mass = 11.86 g/mol
Therefore, the molar mass of the compound is 11.86 g/mol.