The density of CO2 (g) at 25°C and 715 torr is:
P*molar mass = density*RT
1.69g/L
To determine the density of CO2 at a given temperature and pressure, we need to use the ideal gas law equation. The ideal gas law equation is expressed as:
PV = nRT
Where:
P = pressure in atmospheres (atm)
V = volume in liters (L)
n = number of moles (mol)
R = ideal gas constant (0.0821 L atm / K mol)
T = temperature in Kelvin (K)
We need to convert the given temperature to Kelvin:
25°C + 273.15 = 298.15 K
Next, we convert the given pressure from torr to atm:
1 atm = 760 torr
715 torr / 760 torr/atm = 0.9408 atm
Now that we have all the necessary values, rearrange the ideal gas law equation to solve for density:
PV = nRT
Rearranging:
n/V = P/RT
Since we want to find density (d), which is equal to the number of moles (n) divided by volume (V), we can substitute n/V with d:
d = P / RT
Plugging in the values:
d = (0.9408 atm) / (0.0821 L atm / K mol × 298.15 K)
Calculating the result:
d = 0.04002 mol/L
Therefore, the density of CO2 at 25°C and 715 torr is approximately 0.04002 mol/L.