Answer:
V = 12.93 L
Explanation:
Given data:
Number of moles = 0.785 mol
Pressure of balloon = 1.5 atm
Temperature = 301 K
Volume of balloon = ?
Solution:
The given problem will be solve by using general gas equation,
PV = nRT
P= Pressure
V = volume
n = number of moles
R = general gas constant = 0.0821 atm.L/ mol.K
T = temperature in kelvin
Now we will put the values.
V = nRT/P
V = 0.785 mol × 0.0821 atm.L/ mol.K × 301 K / 1.5 atm
V = 19.4 L /1.5
V = 12.93 L
0.785 moles of N₂, fill a balloon at 1.5 atm and 301 K then the volume of the gas is 12.93 L.
Volume of any gas will be used by using an ideal gas equation as:
PV = nRT, where
P = pressure of N₂ gas = 1.5atm
V = volume of N₂ gas = ?
n = moles of N₂ gas = 0.785mol
R = universal gas constant = 0.0821 atm.L/ mol.K
T = temperature of N₂ gas = 301K
On putting values, we get
V = (0.785)(0.0821)(301) / (1.5)
V = 12.93 L
Hence required volume of gas is 12.93L.
To know more about ideal gas equation, visit the below link:
https://brainly.com/question/25290815
