If you need to produce 355 grams of oxygen gas (O2) in the electrolysis reaction of water by an electric current. If the reaction is run at 125 degrees Celsius in a reactor volume 22500ml. What is the pressure of the produced oxygen in mm Hg?
Can't you use PV = nRT and solve for P(in atm) and convert to mm Hg.
n = grams O2/molar mass O2
To find the pressure of the produced oxygen gas (O2), we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in mm Hg)
V = volume of the gas (in liters)
n = number of moles of the gas
R = ideal gas constant (in mmHg·L/mol·K)
T = temperature of the gas (in Kelvin)
First, we need to convert the given reactor volume from mL to L:
22500 mL = 22500/1000 = 22.5 L
Next, we need to convert the given temperature from Celsius to Kelvin:
T = 125 degrees Celsius + 273.15 = 398.15 K
Now, let's calculate the number of moles of oxygen gas produced. We can use the molar mass of oxygen (O2 = 32 g/mol) and the given mass (355 g) to find the number of moles:
n = Mass / Molar mass
n = 355 g / 32 g/mol
n = 11.09375 mol
Since we have all the required values, we can now calculate the pressure of the produced oxygen gas:
P = (n * R * T) / V
Using the values:
n = 11.09375 mol
R = 0.0821 L·atm/(mol·K) (Ideal gas constant)
T = 398.15 K
V = 22.5 L
P = (11.09375 mol * 0.0821 L·atm/(mol·K) * 398.15 K) / 22.5 L
P ≈ 160 mm Hg
Therefore, the pressure of the produced oxygen gas is approximately 160 mm Hg.