What is the pressure of 1.78 g of nitrogen gas confined to a volume of .118 L and 25 degrees Celsius?
To find the pressure of the nitrogen gas, we can use the ideal gas law equation, which is:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = moles of gas
R = ideal gas constant (0.0821 L·atm / (mol·K))
T = temperature (in Kelvin)
First, let's convert the given values to the appropriate units:
Mass of nitrogen gas (m) = 1.78 g
Volume (V) = 0.118 L
Temperature (T) = 25 degrees Celsius = 25 + 273.15 K = 298.15 K
Now, we need to find the number of moles of nitrogen gas using the molar mass of nitrogen gas (N₂).
The molar mass of nitrogen gas (N₂) = 28.0134 g/mol
n = (molar mass) / (mass)
n = 28.0134 g/mol / 1.78 g
n ≈ 15.75 mol
Now, we can substitute the given values into the ideal gas law equation:
(P)(V) = (n)(R)(T)
P = (n)(R)(T) / V
P = (15.75 mol)(0.0821 L·atm / (mol·K))(298.15 K) / 0.118 L
Calculating this expression will give us the pressure (P) of the nitrogen gas confined to a volume of 0.118 L and 25 degrees Celsius.
To find the pressure of the nitrogen gas, we can use the ideal gas law equation: PV = nRT, where P is the pressure, V is the volume, n is the number of moles of gas, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the given temperature from degrees Celsius to Kelvin. We can do this by adding 273.15 to the Celsius value: T = 25 degrees Celsius + 273.15 = 298.15 Kelvin.
Next, we need to calculate the number of moles of nitrogen gas. To do this, we will use the molar mass of nitrogen gas (N₂), which is 28 g/mol.
moles = mass / molar mass
moles = 1.78 g / 28 g/mol
moles ≈ 0.06357 mol (rounded to five decimal places)
Now, we can plug in the values into the ideal gas law equation to find the pressure:
PV = nRT
P * 0.118 L = 0.06357 mol * 0.0821 L·atm/(mol·K) * 298.15 K
Simplifying the equation, we find:
P = (0.06357 mol * 0.0821 L·atm/(mol·K) * 298.15 K) / 0.118 L
Calculating this expression, we find:
P ≈ 1.067 atm (rounded to three decimal places)
Therefore, the pressure of 1.78 g of nitrogen gas confined to a volume of 0.118 L and at a temperature of 25 degrees Celsius is approximately 1.067 atm.
n = grams N2/molar mass N2 = ?
Then use PV = nRT