a. How many moles of N2 are present in a 1.00 qt flask that has a pressure of 425 torr at a temperature of 35°C?
What is the mass in this na2?
It would be much simpler to change quart to liters first, then torr to kpa
PV=nRT
n= PV/RT Temps in Kelvins, V in liters, P in kpa
I did that but I keep getting the wrong answer
To determine the number of moles of N2 present in the flask, we can use the Ideal Gas Law equation:
PV = nRT
Where:
- P is the pressure in atm (converted from torr)
- V is the volume in liters (converted from quarts)
- n is the number of moles of gas
- R is the ideal gas constant (0.0821 L·atm/mol·K)
- T is the temperature in Kelvin (converted from °C)
First, let's convert the given values to the appropriate units:
- Pressure (P): 425 torr = 0.562 atm (since 1 atm = 760 torr)
- Volume (V): 1.00 qt = 0.946 L (since 1 qt = 0.946 L)
- Temperature (T): 35°C + 273.15 = 308.15 K (Kelvin)
Now we can plug these values into the Ideal Gas Law equation:
(0.562 atm)(0.946 L) = n(0.0821 L·atm/mol·K)(308.15 K)
Simplifying the equation:
0.531 atm·L = n(25.385 L·atm/mol)
Dividing both sides of the equation by the coefficient of n:
n = (0.531 atm·L) / (25.385 L·atm/mol)
n ≈ 0.021 moles of N2
Now, to determine the mass of N2, we need to use its molar mass. The molar mass of N2 is approximately 28 grams/mol.
Using the equation:
mass = moles × molar mass
mass = 0.021 moles × 28 g/mol
mass ≈ 0.588 grams
Therefore, the mass of N2 in the given flask is approximately 0.588 grams.