How many mol of nitrogen monoxide gas (N2) are in a 1.49 L container at standard temperature and pressure?
A. 2.14 x 10–24 mol N2
B. 2.89 x 101 mol N2
C. 8.97 x 1023 mol N2
D. 6.65 x 10–2 mol N2
Apparently my last question didnt make sense so i'm hoping this one does
2.89 x 101 mol N2 is not the answer
you know at stp, one mole of any gas occupies 22.4L.
so here, moles=22.4/1.49= and none of the answers are correct. And, Nitrogen monoxide is not N2, it is NO.
Goodness, you have a lot of nonsense questions in your assignment. I hope you don't suffer this often.
Thanks, I have around 8 more mol related questions and then im done with chemistry for the semester so i am just trying to get these right ahh
Did you ever figure out the answer?
To calculate the number of moles of nitrogen monoxide gas (N2) in the given container at standard temperature and pressure, we need to use the ideal gas equation:
PV = nRT
Where:
P = Pressure (in atmospheres)
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), the temperature is 273 K, and the pressure is 1 atmosphere. Given that the volume of the container is 1.49 L, we can plug in the values into the ideal gas equation and solve for the number of moles (n):
(1 atm) * (1.49 L) = n * (0.0821 L·atm/mol·K) * (273 K)
1.49 = n * 0.0821 * 273
n = 1.49 / (0.0821 * 273)
n ≈ 0.0659 mol
Therefore, the number of moles of nitrogen monoxide gas (N2) in the 1.49 L container at standard temperature and pressure is approximately 0.0659 mol.
Among the given options, the closest one to this value is:
D. 6.65 x 10–2 mol N2
So, the answer is D. 6.65 x 10–2 mol N2.