What volume would 10.5 g of nitrogen gas, N2 occupy at 200.K and 2.02 atm.
convert 10.5g N2 to moles.
moles= 10.5/28 as I remember, check it.
V= nRT/P check your R units, to make certain it is in atm
To find the volume of nitrogen gas, N2, we can use the ideal gas law equation:
PV = nRT
Where:
P is the pressure of the gas (in atm)
V is the volume of the gas (in liters)
n is the number of moles of gas
R is the ideal gas constant (0.0821 L.atm/mol.K)
T is the temperature of the gas (in Kelvin)
First, we need to convert the given temperature from Celsius to Kelvin:
200 K = 200 + 273.15 = 473.15 K
We also need to convert the given mass of nitrogen gas into moles. To do this, we need the molar mass of nitrogen gas, which is 28.02 g/mol. Divide the given mass (10.5 g) by the molar mass to get the number of moles:
n = 10.5 g / 28.02 g/mol = 0.374 mol
Now, we can plug the values into the ideal gas law equation:
PV = nRT
(2.02 atm) * V = (0.374 mol) * (0.0821 L.atm/mol.K) * (473.15 K)
Simplifying the equation, we get:
2.02 * V = 0.374 * 0.0821 * 473.15
2.02V = 12.03
Finally, we can solve for V:
V = 12.03 / 2.02
V ≈ 5.96 L
Therefore, 10.5 g of nitrogen gas (N2) would occupy approximately 5.96 liters at 200 K and 2.02 atm.
To solve this problem, we can use the ideal gas law equation:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(K·mol))
T = temperature (in Kelvin)
We have the pressure (P = 2.02 atm), temperature (T = 200 K) and the molar mass of N2 gas (28 g/mol). To find the volume (V), we first need to determine the number of moles (n) using the mass of the gas.
First, find the number of moles (n):
n = mass / molar mass
Given that mass = 10.5 g and the molar mass of N2 = 28 g/mol:
n = 10.5 g / 28 g/mol
n ≈ 0.375 mol
Now we can substitute the known values into the ideal gas law equation and solve for V:
PV = nRT
(2.02 atm) V = (0.375 mol) (0.0821 L·atm/(K·mol)) (200 K)
V = (0.375 mol) (0.0821 L·atm/(K·mol)) (200 K) / (2.02 atm)
V ≈ 7.43 L
Therefore, 10.5 g of nitrogen gas N2 would occupy approximately 7.43 liters at a temperature of 200 K and a pressure of 2.02 atm.