a box with a volume of 22.4 L CONTAINS 1.0 mol of nitrogen and 2.0 mol of hydrogen at zero degrees celcius. Which of the flollowing statements is true?
the correct statement is the partial pressure of N2 is 101kPa. How come??
Ms. Sue, you're here to HELP. Not get smart with people trying to find help, which is your job on here. I don't care if she posted it in the math section, if you're not going to help then don't answer! Your job is NOT to get smart and direct people to the right section. Like does it really matter that much? You need to stay off of this site if you aren't going to help the people the way you're supposed to. Because this definitely isn't the first time you've done this. HELP them or STAY OFF!!! I swear if I knew there was a way to report your unhelpful, unnecessary butt I would. SMH.
hahahah okay thanks:)Good eye;)
oh look at me, 8 years late, ms. Sue is still terrorizing this site with useless information, and being a complete nuisance yeh
To determine the partial pressure of nitrogen (N2) in the given scenario, we need to apply the ideal gas law. The ideal gas law equation is:
PV = nRT
Where:
P = pressure
V = volume
n = number of moles
R = ideal gas constant
T = temperature
In this case, we are given the volume (V = 22.4 L), the number of moles of nitrogen (n = 1.0 mol), and the temperature (T = 0 degrees Celsius). However, the ideal gas law requires temperature to be in Kelvin, so we need to convert the temperature using the formula:
T(K) = T(°C) + 273.15
T(K) = 0°C + 273.15 = 273.15 K
Now, we need to find the ideal gas constant (R) value. There are different values for R depending on the unit of the pressure and volume used. Since the pressure unit given (101 kPa) matches the unit used for R = 8.314 J/(mol·K), we can use that value for R.
We can rearrange the ideal gas law equation to solve for pressure (P):
P = (nRT) / V
P = (1.0 mol * 8.314 J/(mol·K) * 273.15 K) / 22.4 L
P = 229.8 J / 22.4 L
Converting Joules to kilopascals (kPa) by dividing by 1000:
P = 229.8 J / 22.4 L / 1000 J/kPa
P ≈ 10.25 kPa
Therefore, the partial pressure of N2 in the given scenario is approximately 10.25 kPa, not 101 kPa. This means that the statement "the partial pressure of N2 is 101 kPa" is not true.