Assume that the balloon is filled with carbon dioxide gas at 20°C and standard pressure. Use the ideal gas law to calculate the number of moles and mass of CO2 in each balloon at maximum inflation. balloon 1 volume-150.53 balloon 2 volume- 248.47
balloon 3 volume- 463.23
Why did the balloon go to the party? Because it wanted to have a gas-tly good time!
Now, to calculate the number of moles and mass of CO2 in each balloon at maximum inflation, we can use the ideal gas law which is represented as:
PV = nRT
Where:
P = Pressure
V = Volume
n = Number of moles
R = Ideal gas constant
T = Temperature
Assuming standard pressure is 1 atmosphere (atm) and the temperature is 20°C which is 293.15 Kelvin (K), we can calculate the number of moles using the formula:
n = PV / RT
For Balloon 1:
V = 150.53 L
P = 1 atm
T = 293.15 K
Plugging in the values:
n = (1 atm * 150.53 L) / (0.0821 L·atm/mol·K * 293.15 K)
Calculating the result will give us the number of moles in Balloon 1. Similarly, we can repeat the process for Balloon 2 and Balloon 3.
As for the mass of CO2, we would also need the molar mass of carbon dioxide which is approximately 44.01 g/mol. We can then multiply the number of moles by the molar mass to find the mass of CO2 in each balloon.
But hey, speaking of balloons, did you hear about the party they threw for helium balloons? It was off the air!
To calculate the number of moles and mass of CO2 in each balloon at maximum inflation, we'll need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (standard pressure is 1 atm)
V = volume of the balloon
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin (convert 20°C to Kelvin by adding 273.15)
Let's calculate the number of moles and mass of CO2 for each balloon:
Balloon 1:
Volume (V) = 150.53 L
First, let's calculate the number of moles (n):
n = PV / RT
= (1 atm) * (150.53 L) / (0.0821 L·atm/mol·K) * (293.15 K)
≈ 6.11 moles
Now, let's calculate the mass of CO2. We need to know the molar mass of CO2, which is approximately 44 g/mol:
Mass = n * molar mass
= 6.11 moles * 44 g/mol
≈ 269.2 grams
Balloon 2:
Volume (V) = 248.47 L
Using the same calculations as above, we can find:
Number of moles (n) ≈ 10.04 moles
Mass ≈ 441.6 grams
Balloon 3:
Volume (V) = 463.23 L
Again, using the same calculations as above:
Number of moles (n) ≈ 18.87 moles
Mass ≈ 828.7 grams
So, the number of moles and mass of CO2 in each balloon at maximum inflation are approximately:
Balloon 1: 6.11 moles and 269.2 grams
Balloon 2: 10.04 moles and 441.6 grams
Balloon 3: 18.87 moles and 828.7 grams
To calculate the number of moles and mass of CO2 in each balloon at maximum inflation, we can use the ideal gas law. The ideal gas law is given as:
PV = nRT
Where:
P = pressure (in Pascal)
V = volume (in cubic meters)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in Kelvin)
First, we need to convert the volume of each balloon from liters to cubic meters:
Balloon 1 volume: 150.53 L = 0.15053 m³
Balloon 2 volume: 248.47 L = 0.24847 m³
Balloon 3 volume: 463.23 L = 0.46323 m³
Next, we can assume that the standard pressure is 1 atmosphere, which is equivalent to 101325 Pascal. The temperature is given as 20°C, which needs to be converted to Kelvin:
T = 20°C + 273.15 = 293.15 K
Now, we can calculate the number of moles using the ideal gas law. Rearranging the formula, we get:
n = PV / RT
Let's calculate the number of moles and mass of CO2 for each balloon:
For Balloon 1:
P = 101325 Pascal
V = 0.15053 m³
R = 8.314 J/(mol·K)
T = 293.15 K
n₁ = (101325 * 0.15053) / (8.314 * 293.15)
For Balloon 2:
P = 101325 Pascal
V = 0.24847 m³
R = 8.314 J/(mol·K)
T = 293.15 K
n₂ = (101325 * 0.24847) / (8.314 * 293.15)
For Balloon 3:
P = 101325 Pascal
V = 0.46323 m³
R = 8.314 J/(mol·K)
T = 293.15 K
n₃ = (101325 * 0.46323) / (8.314 * 293.15)
To calculate the mass of CO2, we'll need to know the molar mass of carbon dioxide, which is approximately 44.01 g/mol. We can use the equation:
mass = n * molar mass
For Balloon 1:
mass₁ = n₁ * 44.01
For Balloon 2:
mass₂ = n₂ * 44.01
For Balloon 3:
mass₃ = n₃ * 44.01
By calculating these equations, you'll be able to find the number of moles and mass of CO2 gas in each balloon at maximum inflation.
I don't get it. Just use PV = nRT and solve for n. Balloon 1.
P = 1 atm
V = 150.53
n - ?
R = 0.08205
T = 273 + 20 = 293 K
Solve for n = number of mols.
Then grams = n x molar mass = ?