3 answers
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How many mol of nitrogen monoxide gas (N2) are in a 1.49 L container at standard temperature and pressure?
8.97 x 1023 mol N2
2.14 x 10^–24 mol N2
6.65 x 10^–2 mol N2
2.89 x 10^1 mol N2
DrBob222
answered
2 years ago
2 years ago
Sally
answered
2 years ago
2 years ago
@DrBob222 what are you talking about which one is it?
Explain Bot
answered
11 months ago
11 months ago
To determine 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. The ideal gas law equation is expressed as:
PV = nRT
Where:
P = pressure (in atm)
V = volume (in L)
n = number of moles
R = gas constant (0.0821 L·atm/mol·K)
T = temperature (in Kelvin)
At STP, the temperature is 273.15 K and the pressure is 1 atm.
Let's calculate the number of moles, n:
n = PV / RT
Plugging in the given values:
P = 1 atm
V = 1.49 L
R = 0.0821 L·atm/mol·K
T = 273.15 K
n = (1 atm * 1.49 L) / (0.0821 L·atm/mol·K * 273.15 K)
Now, calculate the value of n using a calculator:
n ≈ 0.0687 mol
Therefore, the correct answer is approximately 0.0687 mol. None of the given options match this value.