Answer:
0.779 mol
Explanation:
Since the gas is in a bottle, the volume of the gas is constant. Assuming the temperature remains constant as well, then the gas pressure is proportional to the number of moles:
[tex]p \propto n[/tex]
so we can write
[tex]\frac{p_1}{n_1}=\frac{p_2}{n_2}[/tex]
where
p1 = 730 mm Hg = 0.96 atm is the initial pressure
n1 = 0.650 mol is the initial number of moles
p2 = 1.15 atm is the final pressure
n2 is the final number of moles
Solving for n2,
[tex]n_2 = n_1 \frac{p_2}{p_1}=(0.650 mol)\frac{1.15 atm}{0.96 atm}=0.779 mol[/tex]
Answer: 0.129 moles of gas were added to the bottle
Explanation:
According to the ideal gas equation:'
[tex]PV=nRT[/tex]
P = Pressure of the gas
V= Volume of the gas
T= Temperature of the gas
R= Gas constant
n= moles of gas
As Volume , gas constant and temperature are constant
[tex]\frac{P_1}{n_1}=\frac{P_2}{n _2}[/tex]
where,
[tex]P_1[/tex] = initial pressure of gas =730 mm Hg =0.960 atm (760 mmHg = 1 atm)
[tex]P_2[/tex] = final pressure of gas = 1.15 atm
[tex]n_1[/tex] = initial number of moles = 0.650
[tex]n_2[/tex] = final number of moles = ?
Now put all the given values in the above equation, we get the final moles of gas.
[tex]\frac{0.960}{0.650}=\frac{1.15}{n_2}[/tex]
[tex]n_2=0.779[/tex]
Therefore, the number of moles of gas will be 0.779
Thus moles of gas were added to the bottle are (0.779-0.650) = 0.129
