A Helium Gas Ballon Has A Volume Of 12.0L. At Room Temperature(25 Degrees Celcius) The Internal Pressure Is .05ATM. Calculate The Number Of Moles Of Helium In The Balloon?
To calculate the number of moles of helium in the balloon, we can use the Ideal Gas Law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = number of moles
R = gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
Given:
V = 12.0 L
P = 0.05 atm
T = 25°C = 25 + 273.15 = 298.15 K
Now, we can rearrange the equation to solve for n (number of moles):
n = (PV) / (RT)
Substituting the values:
n = (0.05 atm * 12.0 L) / (0.0821 L·atm/(mol·K) * 298.15 K)
Simplifying, we get:
n = 0.6 / 24.414215
Calculating,
n ≈ 0.0245 mol
Therefore, there are approximately 0.0245 moles of helium in the balloon.
To calculate the number of moles of helium in the balloon, we will use the ideal gas law equation:
PV = nRT
Where:
P is the pressure of the gas (in atm)
V is the volume of the gas (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L·atm/mol·K)
T is the temperature of the gas (in Kelvin)
First, let's convert the temperature from degrees Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 25 + 273.15
T(K) = 298.15 K
Now, rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
Plug in the given values into the equation:
n = (0.05 atm) * (12.0 L) / (0.0821 L·atm/mol·K) * (298.15 K)
n = 0.6 / 24.438
n ≈ 0.0245 moles
Therefore, the number of moles of helium in the balloon is approximately 0.0245 moles.