What is the density of carbon dioxide gas at 25 C and 779 mmHg?
p*molar mass = density x R*T
P is is atm or 779/760 = ?
R = 0.08206 L*atm/mol*K
T = 25C = 298 kelvin
To find the density of carbon dioxide gas at a given temperature and pressure, you can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure
V is the volume
n is the number of moles
R is the ideal gas constant
T is the temperature
Since we are given the temperature (25°C) and pressure (779 mmHg), we can rearrange the ideal gas law equation to solve for density (d):
Density (d) = (P * M) / (R * T)
Where:
M is the molar mass of carbon dioxide, which is 44.01 g/mol
Now, let's plug in the given values and calculate the density:
P = 779 mmHg
T = 25°C (which needs to be converted to Kelvin)
R = 0.0821 L-atm/mol-K
M = 44.01 g/mol
First, we convert the temperature to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 25 + 273.15
T(K) ≈ 298.15 K
Now we can calculate the density:
Density (d) = (P * M) / (R * T)
= (779 mmHg * 44.01 g/mol) / (0.0821 L-atm/mol-K * 298.15 K)
Converting mmHg to atm (since R is in atm):
1 atm = 760 mmHg
So, 779 mmHg = 779/760 atm ≈ 1.024 atm
Density (d) ≈ (1.024 atm * 44.01 g/mol) / (0.0821 L-atm/mol-K * 298.15 K)
≈ 44.91 g/L
Therefore, the density of carbon dioxide gas at 25°C and 779 mmHg is approximately 44.91 g/L.