The density of ethane, C2H6, at 25 oC and 1.10 atm is ___________.
To find the density of ethane (C2H6) at 25°C and 1.10 atm, we need to use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles
R = Gas constant (0.0821 L*atm/(K*mol))
T = Temperature (in Kelvin)
First, let's convert the given temperature from Celsius to Kelvin. The conversion formula is:
T(K) = T(°C) + 273.15
So, T(K) = 25 + 273.15 = 298.15 K
Now, we rearrange the ideal gas law equation to solve for density (d):
V = nRT / P
d = nM / V
Where:
M = Molar mass of ethane (C2H6) is 30.07 g/mol
To find the number of moles (n), we need the mass of ethane. However, this information is not provided in the question. Without the mass, we cannot determine the number of moles and consequently, the density.
Therefore, we cannot calculate the density of ethane (C2H6) at 25°C and 1.10 atm with the given information.
P*molar mass = density*RT
Remember T must be in kelvin.