How many mol of nitrogen monoxide gas (N2) are in a 1.49 L container at standard temperature and pressure?
Use PV = nRT and solve for n. Remember T must be in kelvin. I must point out that nitrogen monoxide is NO and not N2.
To find the number of moles of nitrogen monoxide gas (N2) in a 1.49 L container at standard temperature and pressure, we need to use the ideal gas law formula.
The ideal gas law formula 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)
At standard temperature and pressure (STP):
P = 1 atm
T = 273 K
Since we are given the volume (V) as 1.49 L, we can plug in the values and solve for the number of moles (n).
1 atm * 1.49 L = n * 0.0821 L·atm/mol·K * 273 K
We can simplify this equation by canceling units:
1.49 L = n * 22.4147 L/mol
Now we can solve for n:
n = 1.49 L / 22.4147 L/mol
n ≈ 0.0665 mol
Therefore, there are approximately 0.0665 moles of nitrogen monoxide gas (N2) in a 1.49 L container at standard temperature and pressure.
To calculate the number of moles of nitrogen monoxide gas (N2) in a 1.49 L container at standard temperature and pressure (STP), we can use the ideal gas law equation:
PV = nRT
Where:
P = Pressure (at STP, it is 1 atmosphere)
V = Volume (1.49 liters in this case)
n = Number of moles of gas
R = Ideal Gas Constant (0.0821 L·atm/(mol·K))
T = Temperature (at STP, it is 273.15 K)
First, we need to rearrange the equation to solve for n:
n = (PV) / (RT)
Now, plug in the values:
n = (1 atm * 1.49 L) / (0.0821 L·atm/(mol·K) * 273.15 K)
Calculate the result:
n = 0.0644 moles
Therefore, there are approximately 0.0644 moles of nitrogen monoxide gas (N2) in the 1.49 L container at standard temperature and pressure.