Answer:
5.8 L
Explanation:
Assuming that the hydrogen gas in the balloon acts as an ideal gas, we can solve the problem by using the equation of state for an ideal gas:
[tex]pV=nRT[/tex]
where:
p is the pressure of the gas
V is its volume
n is the number of moles
R is the gas constant
T is the absolute temperature of the gas
For the gas in this problem, we have:
p = 1.05 atm is the pressure
n = 0.24 mol is the number of moles
[tex]T=35^{\circ}C+273=308 K[/tex] is the temperature of the gas
[tex]R=0.082 L \cdot atm\cdot mol^{-1} K^{-1}[/tex] is the gas constant
And solving for V, we find the volume of the gas in liters:
[tex]V=\frac{nRT}{p}=\frac{(0.24)(0.082)(308)}{1.05}=5.8 L[/tex]
Answer:
Its 5.8 Litters.
Explanation:
I took the test on Edmentum/PLATO and got it correct.
