Answer:
1493 balloons.
Explanation:
Hello,
In this case, we first compute the total moles by temperature by using the ideal gas equation as shown below:
[tex]n_{tot}=\frac{PV}{RT}=\frac{200atm*15.0L}{0.082\frac{atm*L}{mol*K}*T}=36585.4mol/T[/tex]
Moreover, since the tank cannot be emptied, we compute the moles that are not transferred:
[tex]n_{not\ transferred}=\frac{1.00atm*15.0L}{0.082\frac{atm*L}{mol*K}*T}=182.93mol/T[/tex]
Now, we compute the moles that are actually transferred:
[tex]n_{transferred}=36585.4mol/T-182.93mol/T=36402.5mol/T[/tex]
Next, since each balloon is filled up to 1.00 atm within a volume of 2.00 L, the moles per balloon are:
[tex]n_{per\ balloon}=\frac{1.00 atm*2.00L}{0.082\frac{atm*L}{mol*K}*T}=24.39mol/T[/tex]
Then, the number of balloons are:
[tex]balloons=\frac{n_{transferred}}{n_{per\ balloon}} =\frac{36402.5mol/T}{24.39mol/T}\\ \\balloons=1492.5\ balloons[/tex]
Which is more accurately 1493 balloons.
Regards.
In the given case, the number of balloons (each 2.00 L) that can be inflated to a pressure of 1.00 atm is -757 ballons.
The ideal gas equation is an important formula in understanding the kinetics of gases.
P1V1 = nRT
In this case, we will use P1V1 = P2V2
then => 102 × 15 = 1 × V2
=> 1530 = v2
=> 1530/ 2 = 765
that means 765 baloons if completely emptied but, here it is mentioned that 1 atm can not be emptied than:
=> 1530 - 15 (the volume of tank is 15 L)
=> 1515/2
=> 757.5
Thus, In the given case, the number of balloons (each 2.00 L) that can be inflated to a pressure of 1.00 atm is -757 ballons.
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