The density of o2 at NTP is 1.429g/l.calcute standard molar volume of gas?
22.4.ltr
a mol of O2 has mass of about 32 g/mol
so 32 g/mol * 1 liter/1.429 g
= (32/1.429) liters/mol
I hope it is about 22.4 liters :)
32/1.429
To calculate the standard molar volume of a gas, we need to use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in Pascals)
V = volume (in cubic meters)
n = number of moles
R = ideal gas constant (8.314 J/(mol⋅K))
T = temperature (in Kelvin)
At standard temperature and pressure (STP), the values are defined as follows:
Pressure (P) = 1 atmosphere = 101,325 Pascals
Temperature (T) = 273.15 Kelvin
We need to find the number of moles (n) of oxygen gas (O2) first:
Given: Density of O2 at NTP = 1.429 g/L
To find the number of moles, we need to convert the given density to grams per cubic meter (g/m^3).
Conversion: 1 g/L = 1000 g/m^3
Therefore, the density of O2 at NTP is 1.429 g/L = 1.429 × 1000 g/m^3 = 1429 g/m^3
Now, let's calculate the number of moles (n) of O2:
Number of moles (n) = Mass / Molar mass
The molar mass of O2 is equal to 32 g/mol (16 g/mol for each oxygen atom).
Now we can calculate the number of moles:
Number of moles (n) = 1429 g/m^3 / 32 g/mol = 44.66 mol/m^3
Next, we can substitute the values into the ideal gas law equation to find the volume (V):
PV = nRT
V = (nRT) / P
Using the values:
Pressure (P) = 101,325 Pa (or 101.325 kPa) - converted to Pascals
Number of moles (n) = 44.66 mol/m^3
Ideal gas constant (R) = 8.314 J/(mol⋅K)
Temperature (T) = 273.15 K
V = (44.66 mol/m^3 * 8.314 J/(mol⋅K) * 273.15 K) / 101,325 Pa
Calculating this expression will give us the standard molar volume of O2 gas.