Answer: a) Partial pressure of argon is 0.673 atm.
b) Partial pressure of ethane is 0.427 atm.
Explanation:
According to the ideal gas equation:'
[tex]PV=nRT[/tex]
P = Pressure of the argon gas = ?
V= Volume of the gas = 1.00 L
T= Temperature of the gas = 25°C = 298 K (0°C = 273 K)
R= Gas constant = 0.0821 atmL/K mol
n= moles of gas = [tex]\frac{\text {given mass}}{\text {Molar mass}}=\frac{1.10g}{40g/mol}=0.0275moles[/tex]
[tex]P=\frac{nRT}{V}=\frac{0.0275\times 0.0821\times 298}{1.00}=0.673atm[/tex]
Thus the partial pressure of argon is 0.673 atm.
b) According to Dalton's law, the total pressure is the sum of individual pressures.
[tex]p_{total}=p_1+p_2[/tex]
[tex]p_{total}=p_{Ar}+p_{ethane}[/tex]
[tex]1.100=0.673+p_{ethane}[/tex]
[tex]1.100-0.673=p_{ethane}[/tex]
[tex]p_{ethane}=0.427atm[/tex]
Thus partial pressure of ethane is 0.427 atm.
