7. Calculate the density of hydrogen sulfide, H2S, at 56 ºC and 967 mmHg. (Express density in g/L)
If you modify the formula for ideal gas (PV = nRT) a little, you'll get an expression for the density of gas:
ρ = P*MM / RT
where
ρ = density (g/L)
P = pressure (atm)
MM = molar mass (g/mol)
R = universal gas constant = 0.0821 L-atm/mol-K
T = absolute temperature (K)
Note that the molar mass of H2S is
2*1 + 1*32 = 34 g/mol
This is a direct substitution, but don't forget to convert the units:
ρ = ((967 / 760) * 34) / (0.0821 * (56 + 273))
Now you can solve for ρ.
hope this helps~ `u`
Well, calculating density involves some serious science and math, but lucky for you, I'm a pro at making serious stuff funny! So, here's my scientific yet humorous answer.
Density is like the superhero of gases, it tells you how tightly packed those gas molecules are in a given space. Now, to calculate the density of hydrogen sulfide (H2S) at 56 ºC and 967 mmHg, we need some facts.
First, I'll assume you've got the molar mass of H2S, which is about 34 grams per mole. Pretty light for a gas, huh? Now, let's get to work!
We'll use the Ideal Gas Law, which goes like this: density = (molar mass x pressure) / (molar volume x temperature)
Now, we know the pressure is 967 mmHg and the temperature is 56 ºC (which is approximately 329 K). But what about molar volume? Well, for gases at low pressures, one mole takes up about 22.4 liters of space. So, let's divide that by 22.4.
Now we have all the ingredients. Let's mix them up and get the density! So, density = (34 g/mol x 967 mmHg) / (22.4 L/mol x 329 K)
After doing some calculations, we find the density of hydrogen sulfide (H2S) at 56 ºC and 967 mmHg is approximately 1.23 g/L. Ta-da!
Remember, science is not just about numbers and formulas, it's also about having a sense of humor. So, let's keep laughing and learning!
To calculate the density of hydrogen sulfide (H2S), we need to use the ideal gas law and the molar mass of H2S.
The ideal gas law is given by the equation:
PV = nRT
Where:
P = Pressure (in atm)
V = Volume (in liters)
n = Number of moles of gas
R = Ideal Gas Constant (0.0821 L.atm/mol.K)
T = Temperature (in Kelvin)
To convert the temperature from ºC to Kelvin, we use the equation:
T (K) = T (ºC) + 273.15
Now, we'll start solving the problem step-by-step:
Step 1: Convert the temperature from ºC to Kelvin
56 ºC + 273.15 = 329.15 K
Step 2: Convert the pressure from mmHg to atm
967 mmHg / 760 mmHg/atm = 1.272 atm
Step 3: Calculate the molar mass of H2S
Molar mass of H = 1.0079 g/mol
Molar mass of S = 32.06 g/mol
Molar mass of H2S = 2(1.0079 g/mol) + 32.06 g/mol = 34.08 g/mol
Step 4: Calculate the density
We can rearrange the ideal gas law equation to solve for density (d):
PV = nRT
n/V = P/RT
Then, we can substitute the molar mass (M) for n and rearrange to solve for density:
d = (M * P) / (R * T)
d = (34.08 g/mol * 1.272 atm) / (0.0821 L.atm/mol.K * 329.15 K)
d = 0.411 g/L
Therefore, the density of hydrogen sulfide (H2S) at 56 ºC and 967 mmHg is approximately 0.411 g/L.
To calculate the density of hydrogen sulfide (H2S) at a given temperature and pressure, you will need to know the molar mass of hydrogen sulfide, the ideal gas law equation, and the molar volume.
Let's break down the steps to get the answer:
Step 1: Find the molar mass of hydrogen sulfide (H2S)
The molar mass of hydrogen (H) is approximately 1.0079 g/mol, and the molar mass of sulfur (S) is approximately 32.06 g/mol. Since we have two hydrogen atoms and one sulfur atom in H2S, we can calculate the molar mass as follows:
Molar mass of H2S = (2 * molar mass of H) + molar mass of S
= (2 * 1.0079 g/mol) + 32.06 g/mol
= 2.0158 g/mol + 32.06 g/mol
= 34.076 g/mol
So, the molar mass of hydrogen sulfide (H2S) is approximately 34.076 g/mol.
Step 2: Apply the ideal gas law equation
The ideal gas law equation is expressed as:
PV = nRT
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
Since we are given the pressure in mmHg, we need to convert it to atm by dividing by the conversion factor of 760 mmHg/atm. In this case, the pressure is given as 967 mmHg, so the pressure in atm will be:
Pressure (atm) = 967 mmHg / 760 mmHg/atm
= 1.272 atm
The temperature is given as 56 ºC. To convert it to Kelvin, we need to add 273.15 to the Celsius value:
Temperature (Kelvin) = 56 ºC + 273.15
= 329.15 K
Step 3: Calculate the molar volume
The molar volume of an ideal gas at a given temperature and pressure is given by:
Molar volume (V) = (R * T) / P
The ideal gas constant (R) is 0.0821 L.atm/(mol.K).
Molar volume (V) = (0.0821 L.atm/(mol.K) * 329.15 K) / 1.272 atm
= 21.258 L/mol
Step 4: Calculate the density
Density is defined as mass per unit volume. Since we know the molar mass and molar volume, we can calculate the density as follows:
Density (g/L) = (Molar mass / Molar volume) * 1000
= (34.076 g/mol / 21.258 L/mol) * 1000
= 1601.145 g/L
Therefore, the density of hydrogen sulfide (H2S) at 56 ºC and 967 mmHg is approximately 1601.145 g/L.