Chemistry Where Did I Go Wrong in My Gas Law Calculation?

AI Thread Summary
The user calculated pressure and volume using the ideal gas law, resulting in a pressure of 146.79 atm and a volume of 0.333 L for argon. However, the error lies in assuming the partial pressure of neon gas equals the total pressure of the gas mixture. In an ideal gas mixture, each gas behaves independently, occupying the entire volume of the container. Therefore, the correct approach requires considering the contributions of all gases to the total pressure. The answer key indicates that the correct volume should be 1 Liter, highlighting the misunderstanding in the calculation.
aboredperson
Messages
1
Reaction score
0
Homework Statement
Given three rigid 1.00-Liter containers at 25o C filled with 1.00 mole of helium gas, 2.00 moles of neon gas, and 3.00 moles of argon gas respectively. When all three gases are pumped into a fourth 1.00-Liter container, what is the volume occupied by the neon gas in the final mixture?
a) 1.00L b) 2.00L c) 3.00L d) 0.167L. E) 0.333L
Relevant Equations
PV=nRT
P=pressure(atm) V= volume (L) n= Moles R= 0.0821 T= Temperature(K)
PV=nRT
P*1L = 6 moles * 0.0821*298 (I added up all the moles and solved for pressure)
P =146.79 atm
146.79 atm * V = 2 moles Ar * 0.0821* 298 (I plugged in the moles for argon and solved for volume)
V= 0.333 L
Answer key says the answer is 1 Liter. Where did I go wrong?
 
Physics news on Phys.org
Looks like you have assumed that partial pressure of the neon gas is the same as the total pressure in the mixture.
 
Last edited:
The 3 gases don't occupy distinct portions of the receiving container separately. They all occupy the complete receiving container. Each gas in an ideal gas mixture behaves as if the other gases are not even present.
 
Thread 'Confusion regarding a chemical kinetics problem'
TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
I don't get how to argue it. i can prove: evolution is the ability to adapt, whether it's progression or regression from some point of view, so if evolution is not constant then animal generations couldn`t stay alive for a big amount of time because when climate is changing this generations die. but they dont. so evolution is constant. but its not an argument, right? how to fing arguments when i only prove it.. analytically, i guess it called that (this is indirectly related to biology, im...
Back
Top