Question

No idea how to solve this. Please help? What is the pressure in a 200.0 mL flask (at T = 27°C) after Ar from a 0.600 L container at 0.600 atm and 227°C is mixed with oxygen from a 0.400 L container at 1.20 atm and 127°C? Assume no reaction takes place between the argon and oxygen.

Answer 1

well im guessing you would just add up pressures by each gas

Answer 2

The answer is 2.88 atm but I dont know how to solve it

Answer 3

wait a sec

Answer 4

yay got it!

Answer 5

alright so
use PV= nRT
to find moles of Ar & O
n= PV / RT
P unit atm
V unit L
R = 0.08206
T unit Kelvin
u have all needed values for both Ar & O to calculate their moles

Answer 6

so, once you get the moles
add them up
and you will get total moles

Answer 7

now use PV= nRT again & this time u will find pressure
P = nRT / V
n= your total mole
R = 0.08206
T = 27 + 273 = K
V = 200 mL / 1000 = L
so use the formula & get your final pressure in atm

Answer 8

I need to find the pressure though, not the moles

Answer 9

ofc, but you need to find moles first

Answer 10

try working out whatever i told you
you will get your answer

Answer 11

Thank you!

Answer 12

no problem :)