How many moles of O2 gas are in a 3700 mL container at a pressure of 1.3 at 33 C?
This is what I have so far
P= 1.3
V= 3700
n= ?
R= 0.0821 atm • L / mio • K
T= 33
But I don’t know how to find the answer
Can someone pls help me
watch your units !
P = 1.3 atm ok I suspect
V = 3700 mL = 3.7 Liters !
T in degrees K = degrees C + 273 = 33+273 = 306 K
P V = n R T
n = P V/ (R T) in mols
To find the number of moles of O2 gas in the given container, you can use the Ideal Gas Law equation:
PV = nRT
where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = gas constant (0.0821 atm ⋅ L/mol ⋅ K)
T = temperature (in Kelvin)
First, let's convert the volume and temperature to the appropriate units.
V = 3700 mL = 3700 mL * (1 L / 1000 mL) = 3.7 L
T = 33 °C = 33 + 273.15 = 306.15 K
Now, we can rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / RT
Substituting the given values:
n = (1.3 atm) * (3.7 L) / (0.0821 atm ⋅ L/mol ⋅ K) * (306.15 K)
Calculating this expression will give you the number of moles of O2 gas in the container.
To find the number of moles (n) of O2 gas in the container, you can use the ideal gas law equation:
PV = nRT
Where:
P = pressure of the gas (in atm)
V = volume of the gas (in liters)
n = number of moles of gas
R = ideal gas constant (0.0821 atm•L / mol•K)
T = temperature of the gas (in Kelvin)
First, you need to convert the given pressure from 1.3 atm to Kelvin by adding 273.15 (since temperature must be in Kelvin):
T = 33 + 273.15 = 306.15 K
Next, convert the given volume from 3700 mL to liters by dividing by 1000:
V = 3700 mL / 1000 = 3.7 L
Now, we can substitute the values into the ideal gas law equation and solve for n:
P * V = n * R * T
(1.3 atm) * (3.7 L) = n * (0.0821 atm•L / mol•K) * (306.15 K)
Simplifying the equation:
4.81 = n * 25.151415
Divide both sides by 25.151415 to solve for n:
n = 4.81 / 25.151415 ≈ 0.191 moles
Therefore, there are approximately 0.191 moles of O2 gas in the 3700 mL container at a pressure of 1.3 atm and a temperature of 33°C.