Using the ideal gas law, the moles of an ideal gas required are
Volume = 1.09 L
Pressure = 1.00 atm
Temperature (not given so we take the room temperature) = 25 °C or 298 K
Value of R = 0.0821 atm.L/mol.K
Number of moles = ?
Ideal gas law:
PV = nRT
Rearrange it for the number of moles (n)
n = PV / RT
Put the values
number of moles (n) = 1.00 atm × 1.09 L ÷ 0.0821 atm.L/mol.K × 298 K
number of moles (n) = 1.09 / 24.46 mol
number of moles (n) = 0.0446 mol
So 0.0446 mol of an ideal gas is required to fill 1.09 L can.
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