What is the mass of nitrogen dioxide contained in a 4.32 L vessel
at 48 °C and 1.40 atm ?
10.5
To calculate the mass of nitrogen dioxide (NO2) contained in a 4.32 L vessel at 48 °C and 1.40 atm, you can use the ideal gas law equation and the molar mass of NO2.
1. Convert temperature from Celsius to Kelvin:
Add 273 to the Celsius temperature to get:
T = 48 °C + 273 = 321 K
2. Determine the number of moles of NO2 using the ideal gas law:
PV = nRT
P: pressure (in atm) = 1.40 atm
V: volume (in L) = 4.32 L
n: number of moles of NO2 (unknown)
R: ideal gas constant = 0.0821 L·atm/mol·K
T: temperature (in K) = 321 K
Rearrange the equation and solve for n:
n = PV / RT
n = (1.40 atm) * (4.32 L) / (0.0821 L·atm/mol·K * 321 K)
3. Calculate the number of moles of NO2:
n ≈ 0.228 mol
4. Find the molar mass of NO2:
The molar mass of NO2 is the sum of the atomic masses of one nitrogen atom (N) and two oxygen atoms (O), which is:
Molar mass of NO2 = (1 * atomic mass of N) + (2 * atomic mass of O)
Use the periodic table to find the atomic masses:
Atomic mass of N = 14.01 g/mol
Atomic mass of O = 16.00 g/mol
Molar mass of NO2 = (1 * 14.01 g/mol) + (2 * 16.00 g/mol) ≈ 46.01 g/mol
5. Calculate the mass of NO2:
Mass = n * molar mass
Mass ≈ 0.228 mol * 46.01 g/mol
Mass ≈ 10.50 g
Therefore, the mass of nitrogen dioxide contained in the 4.32 L vessel at 48 °C and 1.40 atm is approximately 10.50 grams.
To find the mass of nitrogen dioxide (NO2) contained in a 4.32 L vessel at 48 °C and 1.40 atm, we need to use the ideal gas law equation. The ideal gas law equation relates the pressure (P), volume (V), temperature (T), and the number of moles of a gas (n) using the equation: PV = nRT.
Here's how you can calculate it:
1. Convert the temperature from Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 48 + 273.15 = 321.15 K
2. Rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT
3. Convert the volume from liters to cubic meters:
V(m^3) = V(L) / 1000
V(m^3) = 4.32 / 1000 = 0.00432 m^3
4. Use the ideal gas constant (R) value:
R = 0.0821 L · atm/(mol · K) or 8.314 J/(mol · K)
5. Plug the values into the equation to calculate the number of moles:
n = (1.40 atm) * (0.00432 m^3) / (8.314 J/(mol · K) * 321.15 K)
6. Calculate the number of moles (n).
Now that you have the number of moles of nitrogen dioxide in the vessel, you can calculate the mass using the molar mass of nitrogen dioxide (46 g/mol). Multiply the number of moles by the molar mass to obtain the mass.
I hope this helps you find the mass of nitrogen dioxide contained in the given vessel!