Question
Determine the pressure (in atm) of 27.8 g N2 at 35.7 C in 2.40 L. Be sure your answer has the correct number of significant figures.
Note: Reference the Fundamental constants table for additional information.
atm
Note: Reference the Fundamental constants table for additional information.
atm
Answers
GPT 3.5
To find the pressure of the N2 gas, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure
V = volume (in liters)
n = moles of gas
R = ideal gas constant
T = temperature (in Kelvin)
First, we need to find the number of moles of N2:
molar mass of N2 = 28.02 g/mol
moles = mass / molar mass
moles = 27.8 g / 28.02 g/mol
moles = 0.990 moles
Next, we need to convert the temperature to Kelvin:
35.7 C + 273 = 308.7 K
Now we can plug in the values into the ideal gas law equation:
P(2.40 L) = (0.990 moles)(0.08206 L.atm/mol.K)(308.7 K)
P(2.40 L) = 24.1597 atm
P = 24.1597 atm / 2.40 L
P ≈ 10.07 atm
Therefore, the pressure of 27.8 g of N2 gas at 35.7 C in 2.40 L is approximately 10.07 atm. Taking into account significant figures, the answer should be reported as 10 atm.
PV = nRT
Where:
P = pressure
V = volume (in liters)
n = moles of gas
R = ideal gas constant
T = temperature (in Kelvin)
First, we need to find the number of moles of N2:
molar mass of N2 = 28.02 g/mol
moles = mass / molar mass
moles = 27.8 g / 28.02 g/mol
moles = 0.990 moles
Next, we need to convert the temperature to Kelvin:
35.7 C + 273 = 308.7 K
Now we can plug in the values into the ideal gas law equation:
P(2.40 L) = (0.990 moles)(0.08206 L.atm/mol.K)(308.7 K)
P(2.40 L) = 24.1597 atm
P = 24.1597 atm / 2.40 L
P ≈ 10.07 atm
Therefore, the pressure of 27.8 g of N2 gas at 35.7 C in 2.40 L is approximately 10.07 atm. Taking into account significant figures, the answer should be reported as 10 atm.