Answer: a) 0.070 moles of oxygen were produced.
b) New pressure due to the oxygen gas is 2.4 atm
Explanation:
According to ideal gas equation:
[tex]PV=nRT[/tex]
P = pressure of gas = 2.7 atm
V = Volume of gas = 700 ml = 0.7 L
n = number of moles = ?
R = gas constant =[tex]0.0821Latm/Kmol[/tex]
T =temperature = 329 K
[tex]n=\frac{PV}{RT}[/tex]
[tex]n=\frac{2.7atm\times 0.7L}{0.0821 L atm/K mol\times 329K}=0.070moles[/tex]
Thus 0.070 moles of oxygen were produced.
When the 700 mL flask cools to a temperature of 293K.
[tex]PV=nRT[/tex]
[tex]P=\frac{nRT}{V}[/tex]
[tex]P=\frac{0.070\times 0.0821\times 293}{0.7}[/tex]
[tex]P=2.4atm[/tex]
The new pressure due to the oxygen gas is 2.4 atm
