What is the density of hydrogen sulfide (H2S)
at 0.9 atm and 295 K?
Answer in units of g/L
P*molar mass = density*RT
7. Calculate the density of hydrogen sulfide, H2S, at 56 ºC and 967 mmHg. (Express density in g/L)
To find the density of hydrogen sulfide (H2S) at a given pressure and temperature, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = ideal gas constant (0.0821 L · atm / mol · K)
T = temperature (in Kelvin)
To calculate the density, we need to rearrange the ideal gas law equation to solve for density (ρ):
ρ = (n * M) / V
Where:
ρ = density (in g/L)
n = number of moles
M = molar mass of H2S (in g/mol)
V = volume (in L)
First, we need to find the number of moles of H2S. To do that, we divide the given pressure (0.9 atm) by the ideal gas constant (R) multiplied by the given temperature (295 K):
n = (P * V) / (R * T)
n = (0.9 atm * V) / (0.0821 L · atm / mol · K * 295 K)
Secondly, we need to find the molar mass of H2S, which is the sum of the atomic masses of hydrogen (H) and sulfur (S) from the periodic table.
Molar mass of H2S = 2 * (molar mass of H) + (molar mass of S)
Substituting the values of the molar masses:
Molar mass of H2S = 2 * (1.01 g/mol) + 32.07 g/mol
Finally, we substitute the calculated value of the number of moles (n), the molar mass (M), and the formula for density (ρ) into the equation:
ρ = (n * M) / V
Calculating this equation will give us the density of hydrogen sulfide (H2S) at the given conditions of pressure and temperature.