Calculate the density of C2H2 gas (FM = 26.04 g/mol), in g/L, at a pressure of 2.082 atm and at a temperature of 62.5oC.
The general gas law of PV = nRT can be modified to P*molar mass = density*RT.
You can also work it the long way.
PV = nRT and solve for n to find mols. Use 1L for volume.
Then n = grams/molar mass. You know n and molar mass, solve for grams and that will be g/L since you used 1 L for the volume to fine v.
To calculate the density of a gas, we use the ideal gas law, which is given by:
PV = nRT
Where:
P is the pressure in atm
V is the volume in liters
n is the number of moles
R is the ideal gas constant (0.0821 L·atm/(mol·K))
T is the temperature in Kelvin
First, let's convert the given temperature from Celsius to Kelvin:
T (K) = T (°C) + 273.15
T = 62.5 + 273.15
T = 335.65 K
Next, we need to calculate the number of moles (n) of C2H2 gas. To do this, we use the formula:
n = mass / molar mass
Given that the molar mass (FM) of C2H2 is 26.04 g/mol, we need to find the mass. However, we don't have the mass information, so we cannot proceed with this calculation. The density of a gas depends on its mass, so without knowing the mass, we cannot determine the density.
To calculate the density of a gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in L)
n = number of moles of the gas
R = ideal gas constant (0.0821 L · atm/(mol · K))
T = temperature of the gas (in Kelvin)
To use this equation, we need to convert the temperature from Celsius to Kelvin:
T(K) = T(C) + 273.15
T(K) = 62.5 + 273.15 = 335.65 K
First, we need to calculate the volume using the ideal gas law equation:
V = (nRT) / P
To find the number of moles (n), we can use the formula:
n = mass / molar mass
So, to calculate the number of moles, we need to know the mass of the gas.
However, we don't have the mass of the gas given in the question. Without the mass, we can't proceed with the calculation. Could you provide the mass of the gas?