What is the volume of a gas tank which contains 10.4 g of nitrogen gas a 2 g and 4.50 atm?
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What is the volume of a gas tank which contains 10.4 g of nitrogen gas at 25C and 4.50 atm?
Convert 10.4 g N2 to moles (moles = grams/molar mass) and use PV =nRT
To find the volume of the gas tank, you can use the ideal gas law equation, which states:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in liters)
n = moles of gas
R = ideal gas constant (0.0821 L * atm / (mol * K))
T = temperature (in Kelvin)
We are given the following information:
n = 10.4 g of nitrogen gas
P = 2.50 atm
T = unknown
First, we need to convert grams of nitrogen gas to moles. To do this, we divide the mass of the gas by its molar mass.
The molar mass of nitrogen gas (N₂) is 28 g/mol (14 g/mol per nitrogen atom * 2 nitrogen atoms in N₂).
Moles = mass / molar mass
Moles = 10.4 g / 28 g/mol
Moles ≈ 0.371 mol
Now, we have the moles of gas (n) and the pressure (P), but we need to find the volume (V). To do this, we rearrange the ideal gas law equation:
V = (nRT) / P
Since we need to find the volume in liters, we need to convert the temperature to Kelvin. Let's assume the temperature is 25°C.
T(K) = T(°C) + 273
T(K) = 25 + 273
T(K) = 298 K
Now we can substitute the values into the equation:
V = (0.371 mol * 0.0821 L * atm / (mol * K) * 298 K) / 2.50 atm
Calculating this equation will give us the volume (V) in liters:
V = (0.0305055118 L) / (2.50 atm)
V ≈ 0.0122 L
Therefore, the volume of the gas tank is approximately 0.0122 liters.