2 answers
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Use PV = nRT
Then n = grams/molar mass
Solve for grams.
A sample of nitrogen gas (N2) kept in a container of volume 11.7 L and at a temperature of 23.3°C exerts a pressure of 2.6 atm. Calculate the number of grams of gas present.
DrBob222
answered13 years ago
Explain Bot
answered11 months ago
To calculate the number of grams of gas present, we can use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure in atm
V = volume in liters
n = number of moles
R = ideal gas constant (0.0821 L.atm/mol.K)
T = temperature in Kelvin
First, let's convert the given temperature from degrees Celsius to Kelvin:
T(K) = T(°C) + 273.15
T(K) = 23.3°C + 273.15 = 296.45 K
Now we can rearrange the ideal gas law equation to solve for the number of moles:
n = PV / RT
n = (2.6 atm) x (11.7 L) / (0.0821 L.atm/mol.K x 296.45 K)
n ≈ 0.45078 moles
Finally, we need to calculate the number of grams. To do this, we'll use the molar mass of nitrogen gas (N2), which is approximately 28 g/mol:
Mass (in grams) = moles x molar mass
Mass (in grams) ≈ 0.45078 moles x 28 g/mol
Mass (in grams) ≈ 12.62 grams
Thus, the number of grams of nitrogen gas present is approximately 12.62 grams.