How many milligrams of a mixture containing equal numbers of moles of CH4 and N2 at 10 ATM total pressure will dissolve in 1 L of water at 20°C
??? Convert 16g/mol CH4 28g/mol N2
???need density .998g/ml H2O
You need to use Henry's Law. You will need the constants for each.
Ok 24mg/100g and 18mg/100g from graph
I'm not sure what to do with the .018 and .024 o even have the answer from the book.
To determine the number of milligrams of the mixture that will dissolve in 1 L of water at 20°C, we need to calculate the number of moles of CH4 and N2 in the mixture.
First, we need to find the total number of moles of gas in the mixture. Since the mixture contains an equal number of moles of CH4 and N2, we only need to calculate the moles of one of the gases.
Given:
Molar mass of CH4 = 16 g/mol
Molar mass of N2 = 28 g/mol
Next, we'll convert the pressure from atmospheres (ATM) to moles using the ideal gas law:
PV = nRT
Where:
P = pressure in atmospheres
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L·atm/mol·K)
T = temperature in Kelvin
Given:
Total pressure (P) = 10 ATM
Volume (V) = 1 L
Temperature (T) = 20°C = 293.15 K
Using the ideal gas law, we can calculate the total number of moles (n) in the mixture:
n = PV / RT
n = (10 ATM * 1 L) / (0.0821 L·ATM/mol·K * 293.15 K)
n ≈ 0.407 moles
Since the mixture contains an equal number of moles of CH4 and N2, we can divide the total number of moles (0.407 moles) by 2 to get the moles of each gas:
0.407 moles / 2 = 0.204 moles (approx.)
Now, we can calculate the mass of each gas using their respective molar masses:
Mass of CH4 = number of moles * molar mass
Mass of CH4 = 0.204 moles * 16 g/mol
Mass of CH4 ≈ 3.264 g
Mass of N2 = number of moles * molar mass
Mass of N2 = 0.204 moles * 28 g/mol
Mass of N2 ≈ 5.712 g
To convert the mass of the mixture into milligrams, we multiply by 1000:
Mass of mixture = Mass of CH4 + Mass of N2
Mass of mixture = 3.264 g + 5.712 g
Mass of mixture ≈ 8.976 g ≈ 8976 mg
Therefore, approximately 8976 milligrams of the mixture containing equal numbers of moles of CH4 and N2 at 10 ATM total pressure will dissolve in 1 L of water at 20°C.
Additional information: The given density of water, 0.998 g/mL, is not needed to calculate the number of milligrams of the mixture that will dissolve in water.