July 19, 2024, 12:06:09 PM
Forum Rules: Read This Before Posting


Topic: Gas Equilibrium Question  (Read 1517 times)

0 Members and 1 Guest are viewing this topic.

Offline YourWorstNightmare

  • Very New Member
  • *
  • Posts: 1
  • Mole Snacks: +0/-0
Gas Equilibrium Question
« on: June 13, 2015, 07:53:55 PM »
Okay, my understanding of gas equilibrium systems is that if a given system is at equilibrium, and then you increase the pressure the equilibrium will shift in the direction that has fewer gas molecules (which makes complete sense to me), and vice versa.

When given the equilibrium system as follows:

Methane (g) + Water (g) + 20.50 kJ  ::equil:: Carbon Monoxide (g) + 3 Hydrogen (g)

And told that the pressure was increased by adding an inert gas, since there was 4 gas molecules on the right side and 2 on the left I assumed that the reaction would then shift in the left direction and that [CO] would decrease.  However, I wrote that on a test and it was incorrect.

I figured I should get to the bottom of it before I saw the exact same question on the exam.

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27747
  • Mole Snacks: +1804/-411
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Gas Equilibrium Question
« Reply #1 on: June 14, 2015, 02:38:14 AM »
Equilibrium depends on the partial pressures of gases. When you add an inert gas total pressure changes, but partial pressures of the compounds involved in the equilibrium do not.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Sponsored Links