if 10.0L of neon gas exerts a pressure of 125psi at 373K, what is the number of moles of gas?
I don't know how to set this up. I am using ideal gas law N=PV/RT but my answer is not matching.
I converted the 125psi to 8.50atm
N= 8.50atm*10.0L/1 k * 373k*1 mol/1 atm * 0.0821 L
Where am I going wrong?
N=PV/RT=8.5*10/(.00821*373)=about 27 moles
Maybe you have temp in the numberator?
Here's where you went wrong in setting up the calculation. Although you correctly converted the pressure from 125 psi to 8.50 atm, you made a mistake in the conversion factor for the ideal gas constant (R).
The value of the ideal gas constant is 0.0821 L·atm/(mol·K), not 0.0821 L.
So the correct setup of the equation would be:
N = (P * V) / (R * T)
N = (8.50 atm * 10.0 L) / (0.0821 L·atm/(mol·K) * 373 K)
Simplifying:
N = 85.0 / (0.0821 * 373)
N ≈ 2.39 moles
So, the correct number of moles of gas is approximately 2.39 moles.