Answer:
The volume inside the balloon is = 121 [tex]m^{3}[/tex]
Explanation:
Temperature T = - 1 °c = 272 K
Pressure = 0.7 atm = 71 k pa
No. of moles = 3.8
Mass of the gas inside the volume = 3.8 × 4 = 15.2 kg
From ideal gas equation
P V = m R T
Put all the values in above formula we get
71 × V =15.2 × 2.077 × 272
V = 121 [tex]m^{3}[/tex]
Therefore the volume inside the balloon is = 121 [tex]m^{3}[/tex]
Answer:
[tex]\large \boxed{\text{121 L}}[/tex]
Explanation:
We can use the Ideal Gas Law.
pV = nRT
Data:
p = 0.700 atm
n = 3.80 mol
T = -1 °C
Calculations:
1. Convert the temperature to kelvins
T = (-1 + 273.15) K= 272.15 K
2. Calculate the volume
[tex]\begin{array}{rcl}pV &=& nRT\\\text{0.700 atm} \times V & = & \text{3.80 mol} \times \text{0.082 06 L}\cdot\text{atm}\cdot\text{K}^{-1}\text{mol}^{-1} \times \text{272.15 K}\\0.700V & = & \text{84.86 L}\\V & = & \textbf{121 L} \\\end{array}\\\text{The volume of the balloon is $\large \boxed{\textbf{121 L}}$}[/tex]
