Here's the question you clicked on:

55 members online
  • 0 replying
  • 0 viewing

yrelhan4

  • 3 years ago

SO3(g) decomposes according to the equation 2SO3(g) → 2SO2(g) + O2(g) A sealed container contains 0.50 mol of SO3 gas at 100°C and 2 atmospheres pressure. What would be the pressure in the container if the SO3 gas is decomposed completely according to the above equation and the temperature were maintained at 100°C ?

  • This Question is Closed
  1. olzha.y
    • 3 years ago
    Best Response
    You've already chosen the best response.
    Medals 1

    Because its a sealed container its volume is constant + and temperature is also constant: PV = nRT => V/RT = contstant too.. 2SO3 => 2SO2 + O2 0.5 mole 0.5 mole 0.25 mole V/RT = constant = n(initial)/P(initial) = n(final)/P(final) n(inital) = n(SO3) = 0.5 mole, P(initial) = 2atm, n(final) = n(SO2) + n(O2) => 0.5 mole + 0.25 mole = 0.75 mole, P(final) = x atm n(inital)/P(initial) = 0.5 mole/2 atm = 0.75 mole / x atm => 0.5x = 1.5 => x = 3 atm = P(final)

  2. Not the answer you are looking for?
    Search for more explanations.

    • Attachments:

Ask your own question

Sign Up
Find more explanations on OpenStudy
Privacy Policy